Energetics Q + MS

7/27/2019 Energetics Q + MS

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1. What energy changes occur when chemical bonds are formed and broken?

A. Energy is absorbed when bonds are formed and when they are broken.

B. Energy is released when bonds are formed and when they are broken.

C. Energy is absorbed when bonds are formed and released when they are broken.

D. Energy is released when bonds are formed and absorbed when they are broken.

2. The temperature of a 2.0 g sample of aluminium increases from 25C to 30C.

How many joules of heat energy were added? (Specific heat of Al = 0.90 J g1

K1

)

A. 0.36 B. 2.3 C. 9.0 D. 11

3. Using the equations below:

C(s) + O2(g) CO2(g) H=390 kJ

Mn(s) + O2(g) MnO2(s) H=520 kJ

what is H(in kJ) for the following reaction?

MnO2(s) + C(s) Mn(s) + CO2(g)

A. 910 B. 130 C. 130 D. 910

4. Under what circumstances is a reaction spontaneous at all temperatures?

H S

A. + +

B. +

C.

D. +

5. Which combination of ionic charge and ionic radius give the largest lattice enthalpy for an ionic

compound?

Ionic charge Ionic radius

A. high large

B. high small

C. low small

D. low large

6. What is Hfor the reaction below in kJ?

CS2(g) + 3O2(g) CO2(g) + 2SO2(g)

[Hf/kJ mol1

: CS2(g) 110, CO2(g)390, SO2(g)290]

A. 570 B. 790 C. 860 D. 1080

7. Which statements about exothermic reactions are correct?

I. They have negative Hvalues.


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II. The products have a lower enthalpy than the reactants.

III. The products are more energetically stable than the reactants.

A. I and II only B. I and III only

C. II and III only D. I, II and III

8. A sample of a metal is heated. Which of the following are needed to calculate the heat absorbedby the sample?

I. The mass of the sample

II. The density of the sample

III. The specific heat capacity of the sample



9. The average bond enthalpies for OO and O==O are 146 and 496 kJ mol1

respectively.

What is the enthalpy change, in kJ, for the reaction below?

HOOH(g) HOH(g) + O==O(g)

A. 102 B. + 102 C. + 350 D. + 394

10. Which reaction has the greatest positive entropy change?

A. CH4(g) + 1O2(g) CO(g) + 2H2O(g)

B. CH4(g) + 1O2(g) CO(g) + 2H2O(l)

C. CH4(g) + 2O2(g) CO2(g) + 2H2O(g)

D. CH4(g) + 2O2(g) CO2(g) + 2H2O(l)

11. What is the energy change (in kJ) when the temperature of 20 g of water increases by 10C?

A. 20104.18 B. 202834.18

C.1000

18.41020

D.

100018.428320

12. The lattice enthalpy values for lithium fluoride and calcium fluoride are shown below.

LiF(s) H = +1022 kJ mol1

CaF2(s) H

= +2602 kJ mol1

Which of the following statements help(s) to explain why the value for lithium fluoride is lessthan that for calcium fluoride?

I. The ionic radius of lithium is less than that of calcium.

II. The ionic charge of lithium is less than that of calcium.

A. I only B. II only C. I and II D. Neither I nor II

13. When the solids Ba(OH)2 and NH4SCN are mixed, a solution is produced and the

temperature drops.


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Ba(OH)2(s) + 2NH4SCN(s) Ba(SCN)2(aq) + 2NH3(g) + 2H2O(l)

Which statement about the energetics of this reaction is correct?

A. The reaction is endothermic and His negative.

B. The reaction is endothermic and His positive.

C. The reaction is exothermic and His negative.

D. The reaction is exothermic and His positive.

14. Using the equations below

Cu(s) +21 O2(g) CuO(s)H

=156 kJ

2Cu(s) +21 O2(g) Cu2O(s)H

=170 kJ

what is the value ofH

(in kJ) for the following reaction?

2CuO(s) Cu2O(s) + 21

O2(g)

A. 142 B. 15 C. 15 D. 142

15. Which reaction occurs with the largest increase in entropy?

A. Pb(NO3)2(s) + 2KI(s) PbI2(s) + 2KNO3(s)

B. CaCO3(s) CaO(s) + CO2(g)

C. 3H2(g) + N2(g) 2NH3(g) D. H2(g) + I2(g) 2HI(g)

16. The H and Svalues for a certain reaction are both positive. Which statement is correctabout the spontaneity of this reaction at different temperatures?

A. It will be spontaneous at all temperatures.

B. It will be spontaneous at high temperatures but not at low temperatures.

C. It will be spontaneous at low temperatures but not at high temperatures.

D. It will not be spontaneous at any temperature.

17. Which of the quantities in the enthalpy level diagram below is (are) affected by the use of acatalyst?

I II

III

Enthalpy

Time


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A. I only B. III only C. I and II only D. II and III only

18. Which reaction has the most negative H value?

A. LiF(s) Li+(g) + F

(g) B. Li

+(g) + F

(g) LiF(s)

C. NaCl(s) Na+(g) + Cl(g) D. Na+(g) + Cl(g) NaCl(s)

19. Consider the following equations.

Mg(s) +21 O2(g) MgO(s) H

=602 kJ

H2(g) + 21 O2(g) H2O(g) H

=242 kJ

What is the H value (in kJ) for the following reaction?

MgO(s) + H2(g) Mg(s) + H2O(g)

A. 844 B. 360 C. +360 D. +844

20. For which of the following is the sign of the enthalpy change different from the other three?

A. CaCO3(s) CaO(s) + CO2(g) B. Na(g) Na+(g) + e

C. CO2(s) CO2(g) D. 2Cl(g) Cl2(g)

21. Which reaction has a positive entropy change, S?

A. H2O(g) H2O(l) B. 2SO2(g) + O2(g) 2SO3(g)

C. CaCO3(s) CaO(s) + CO2(g) D. N2(g) + 3H2(g) 2NH3(g)

22. Separate solutions of HCl(aq) and H2SO4(aq) of the same concentration and same volume

were completely neutralized by NaOH(aq).XkJ and YkJ of heat were evolved respectively.

Which statement is correct?

A. X= Y B. Y= 2X C. X= 2Y D. Y= 3X

23. Which statements are correct for an endothermic reaction?

I. The system absorbs heat.

II. The enthalpy change is positive.

III. The bond enthalpy total for the reactants is greater than for the products.



24. The mass m (in g) of a substance of specific heat capacity c (in J g1

K1

) increases by tC.What is the heat change in J?

A. mct B. mc(t+ 273) C.1000mct

D.

1000

)273( tmc

25. The average bond enthalpy for the CH bond is 412 kJ mol1

. Which process has an enthalpychange closest to this value?


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A. CH4(g) C(s) + 2H2(g) B. CH4(g) C(g) + 2H2(g)

C. CH4(g) C(s) + 4H(g) D. CH4(g) CH3(g) + H(g)

26. For a certain reaction at 298 K the values of both Hand Sare negative. Which statement

about the sign ofG for this reaction must be correct?

A. It is negative at all temperatures.

B. It is positive at all temperatures.

C. It is negative at high temperatures and positive at low temperatures.

D. It cannot be determined without knowing the temperature.

27. Which type of reaction is referred to in the definition ofstandard enthalpy change of formation?

A. the formation of a compound from its elements

B. the formation of a crystal from its ions

C. the formation of a molecule from its atoms

D. the formation of a compound from other compounds

28. The following equation shows the formation of magnesium oxide from magnesium metal.

2Mg(s) + O2(g)2MgO(s) H =1204kJ

Which statement is correct for this reaction?

A. 1204 kJ of energy are released for every mol of magnesium reacted.

B. 602 kJ of energy are absorbed for every mol of magnesium oxide formed.

C. 602 kJ of energy are released for every mol of oxygen gas reacted.

D. 1204 kJ of energy are released for every two mol of magnesium oxide formed.

29. The following equations show the oxidation of carbon and carbon monoxide to carbon dioxide.

C(s) +O2(g) CO2(g) H =x kJ mol1

CO(g) +21 O2(g) CO2(g) H

=y kJ moll

What is the enthalpy change, in kJ mol1, for the oxidation of carbon to carbon monoxide?

C(s) +21 O2(g) CO(g)

A. x +y B. xy C. yx D. xy

30. A simple calorimeter was used to determine the enthalpy of combustion of ethanol. The

experimental value obtained was920 kJ mol1. The Data Booklet value is1371 kJ mol1.

Which of the following best explains the difference between the two values?

A. incomplete combustion of the fuel B. heat loss to the surroundings

C. poor ventilation in the laboratory D. inaccurate temperature

measurements


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31. What is the correct order of decreasing entropy for a pure substance?

A. gas liquid solid B. solid liquid gas

C. solid gas liquid D. liquid solid gas

32. For the reaction

2H2(g) + O2(g) 2H2O(g)

the bond enthalpies (in kJ mol1) are

HH x

O=O y

OH z

Which calculation will give the value, in kJ mol1, ofH for the reaction?

A. 2x +y2z B. 4z2xy

C. 2x +y4z D. 2z2xy

33. Which statement about bond enthalpies is correct?

A. Bond enthalpies have positive values for strong bonds and negative values for weakbonds.

B. Bond enthalpy values are greater for ionic bonds than for covalent bonds.

C. Bond breaking is endothermic and bond making is exothermic.

D. The carboncarbon bond enthalpy values are the same in ethane and ethene.

34. An equation for a reaction in which hydrogen is formed is

CH4 + H2O 3H2 + CO H = +210 kJ

Which energy change occurs when 1 mol of hydrogen is formed in this reaction?

A. 70 kJ of energy are absorbed from the surroundings.

B. 70 kJ of energy are released to the surroundings.

C. 210 kJ of energy are absorbed from the surroundings.

D. 210 kJ of energy are released to the surroundings.

35. The equations and enthalpy changes for two reactions used in the manufacture of sulfuric acidare:

S(s) + O2(g) SO2(g) H

=300 kJ

2SO2(g) + O2(g) 2SO3(g) H =200 kJ

What is the enthalpy change, in kJ, for the reaction below?

2S(s) + 3O2(g) 2SO3(g)

A. 100 B. 400 C. 500 D. 800


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36. Which reaction has the largest positive value ofS?

A. CO2(g) + 3H2(g) CH3OH(g) + H2O(g) B. 2Al(s) + 3S(s) Al2S3(s)

C. CH4(g) + H2O(g) 3H2(g) + CO(g) D. 2S(s) + 3O2(g) 2SO3(g)

37. Approximate values of the average bond enthalpies, in kJ mol1

, of three substances are:

HH 430

FF 155

HF 565

What is the enthalpy change, in kJ, for this reaction?

2HF H2 + F2

A. +545 B. +2 C. 20 D. 545

38. The standard enthalpy change of formation values of two oxides of phosphorus are:

P4(s) + 3O2(g) P4O6(s) H

f=1600 kJ mol1

P4(s) + 5O2(g) P4O10(s) H

f=3000 kJ mol1

What is the enthalpy change, in kJ mol1

, for the reaction below?

P4O6(s) + 2O2(g) P4O10(s)

A. +4600 B. +1400 C. 1400 D. 4600

39. Which is a correct equation to represent the lattice enthalpy of magnesium sulfide?

A. MgS(s) Mg(s) + S(s) B. MgS(s) Mg(g) + S(g)

C. MgS(s) Mg+(g) + S(g) D. MgS(s) Mg

2+(g) + S2(g)

40. Which equation represents a change with a negative value forS?

A. 2H2(g) + O2(g) 2H2O(g) B. H2O(s) H2O(g)

C. H2(g) + Cl2(g) 2HCl(g) D. 2NH3(g) N2(g) + 3H2(g)

41. The expression for the standard free energy change of a reaction is given by

G = H

TS

What are the signs forH and S for a reaction that is spontaneous at all temperatures?

H S

A. +

B. +

C. + +

D.


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42. Which statement is correct for an endothermic reaction?

A. The products are more stable than the reactants and His positive.

B. The products are less stable than the reactants and His negative.

C. The reactants are more stable than the products and His positive.

D. The reactants are less stable than the products and His negative.

43. Which statement is correct about the reaction shown?

2SO2(g) + O2(g) 2SO3(g) H=196 kJ

A. 196 kJ of energy are released for every mole of SO2(g) reacted.

B. 196 kJ of energy are absorbed for every mole of SO2(g) reacted.

C. 98 kJ of energy are released for every mole of SO2(g) reacted.

D. 98 kJ of energy are absorbed for every mole of SO2(g) reacted.

44. Which statements are correct for all exothermic reactions?

I. The enthalpy of the products is less than the enthalpy of the reactants.

II. The sign ofHis negative.

III. The reaction is rapid at room temperature.

A. I and II only B. I and III onl C. II and III only D. I, II and III

45. Which are characteristics of ions in an ionic compound with a large lattice enthalpy value?

A. Large ionic radius and high ionic charge

B. Small ionic radius and low ionic charge

C. Large ionic radius and low ionic charge

D. Small ionic radius and high ionic charge

46. Consider the specific heat capacity of the following metals.

Metal Specific heat capacity / J kg1

K1

Cu 385

Ag 234

Au 130

Pt 134

Which metal will show the greatest temperature increase if 50 J of heat is supplied to a 0.001 kgsample of each metal at the same initial temperature?

A. Cu B. Ag C. Au D. Pt

47. Consider the following reactions.


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S(s) + 211 O2(g) SO3(g) H

= 395 kJ mol1

SO2(s) + 21 O2(g) SO3(g) H

= 98 kJ mol1

What is the H value (in kJ mol1) for the following reaction?

S(s) + O2(g) SO2(g)

A. 297 B. +297 C. 493 D. +493

48. The following reaction is spontaneous only at temperatures above 850C.

CaCO3(s) CaO(s) + CO2(g)

Which combination is correct for this reaction at 1000C?

G H S

A.

B. + + +

C. + +

D. +

49. Which statement is correct for an endothermic reaction?

A. Bonds in the products are stronger than the bonds in the reactants.

B. Bonds in the reactants are stronger than the bonds in the products.

C. The enthalpy of the products is less than that of the reactants.

D. The reaction is spontaneous at low temperatures but becomes non-spontaneous at hightemperatures.

50. Consider the following information.

Compound C6H6(l) CO2(g) H2O(l)

Hf / kJ mol1 +49 +394 286

C6H6(l) + 217 O2(g) 6CO2(g) + 3H2O(l)

Which expression gives the correct value of the standard enthalpy change of combustion forbenzene (l), in kJ mol

1?

A. 12(394) + (286) 2(49) B. 12(394) + 6(286) 2(49)

C. 6(394) + 3(286) (49) D. 6(394) + 3(286) (49)

51. Which equation represents the lattice enthalpy of magnesium oxide?

A. Mg(s) +2

1 O2(g) MgO(s) B. Mg2+(g) + O2(g) MgO(g)

C. Mg2+

(g) + 21

O2(g) MgO(s) D. Mg2+

(g) + O2

(g) MgO(s)

52. According to the enthalpy level diagram below, what is the sign forHand what term is used to


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refer to the reaction?

H

reaction progress

reactants

products

H reaction

A. positive endothermic

B. negative exothermic

C. positive exothermic

D. negative endothermic

53. When 40 joules of heat are added to a sample of solid H2O at16.0C the temperature increases

to8.0C. What is the mass of the solid H2O sample? [Specific heat capacity of H2O(s) = 2.0 J

g1K1]

A. 2.5 g B. 5.0 g C. 10 g D. 160 g

54. The H values for the formation of two oxides of nitrogen are given below.

2

1

N2(g) + O2(g) NO2(g) H

=57 kJ mol1

N2(g) + 2O2(g) N2O4(g) H = +9 kJ mol1

Use these values to calculate H

for the following reaction (in kJ):

2NO2(g) N2O4(g)

A. 105 B. 48 C. +66 D. +123

55. The H and S

values for a reaction are both negative. What will happen to the spontaneity

of this reaction as the temperature is increased?

A. The reaction will become more spontaneous as the temperature is increased.

B. The reaction will become less spontaneous as the temperature is increased.

C. The reaction will remain spontaneous at all temperatures.

D. The reaction will remain non-spontaneous at any temperature.

56. How much energy, in joules, is required to increase the temperature of 2.0 g of aluminium from

25 to 30C? (Specific heat of Al = 0.90 J g1

K1

).

A. 0.36 B. 4.5 C. 9.0 D. 54


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57. Which combination is correct for a chemical reaction that absorbs heat from the surroundings?

Type of reaction Hat constant pressure

A. Exothermic Positive

B. Exothermic Negative

C. Endothermic Positive

D. Endothermic Negative

58. Using the equations below:

C(s) + O2(g) CO2(g) H =394 kJ mol1

Mn(s) + O2(g) MnO2(s) H =520 kJ mol1

What is H, in kJ, for the following reaction?

MnO2(s) + C(s) Mn(s) + CO2(g)

A. 914 B. 126 C. 126 D. 914

59. Which reaction has the most negative H

value?

A. LiF(s) Li+(g) + F(g) B. Li+(g) + F(g) LiF(s)

C. NaCl(s) Na+(g) + Cl(g) D. Na+(g) + Cl(g) NaCl(s)

60. Which equation represents the electron affinity of calcium?

A. Ca(g) Ca+(g) + e B. Ca(g) Ca(g) + e

C. Ca(g) + e Ca(g) D. Ca+(g) + e Ca(g)

61. Which reaction causes a decrease in the entropy of the system?

A. CaCO3(s) CaO(s) + CO2(g) B. 2H2(g) + O2(g) 2H2O(l)

C. 2C(s) + O2(g) 2CO(g) D. 2SO3(g) 2SO2(g) + O2(g)

62. What are the signs ofH

and S

for a reaction that is non-spontaneous at low temperature butspontaneous at high temperature?

H SA.

B. +

C. +

D. + +

63. Given the following data:

C(s) + F2(g) CF4(g); H1=680 kJ mol1

F2(g) 2F(g); H2= +158 kJ mol1

C(s) C(g); H3= +715 kJ mol

1


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calculate the average bond enthalpy (in kJ mol1

) for the CF bond.

64. For the process: C6H6(l) C6H6(s)

the standard entropy and enthalpy changes are:

H=9.83kJ mol1 and S=35.2J K1 mol1.

Predict and explain the effect of an increase in temperature on the spontaneity of the process.

65. Explain in terms ofG, why a reaction for which both H andS values are positive cansometimes be spontaneous and sometimes not.

66. Consider the following reaction. N2(g) +3H2(g) 2NH3(g)

(i) Use values from Table 10 in the Data Booklet to calculate the enthalpy change, H, for

this reaction.

(ii) The magnitude of the entropy change, S, at 27C for the reaction is 62.7 J K1

mol1

.

State, with a reason, the sign ofS. (2)

(iii) Calculate G for the reaction at 27C and determine whether this reaction is spontaneousat this temperature.

67. Explain in terms ofG, why a reaction for which bothH

and S are positive is sometimes

spontaneous and sometimes not.

68. Consider the following reaction.

N2(g) + 3H2(g) 2NH3(g)

(i) Using the average bond enthalpy values in Table 10 of the Data Booklet, calculate the

standard enthalpy change for this reaction. (4)

(ii) The absolute entropy values, S, at 300 K for N2(g), H3(g) and NH2(g) are 193, 131 and

192 JK1 mol1 respectively. Calculate S for the reaction and explain the sign ofS

.

iii) Calculate G for the reaction at 300 K.

(iv) If the ammonia was produced as a liquid and not as a gas, state and explain the effect this

would have on the value ofH for the reaction.(2)

69. Define the termstandard enthalpy of formation, and write the equation for the standard enthalpy

of formation of ethanol.

70. Two reactions occurring in the manufacture of sulfuric acid are shown below:

reaction I S(s) +O2(g) SO2(g) H =297 kJ

reaction II SO2(g) + 21 O2(g) SO3(g) H

=92 kJ

(i) State the name of the term H. State, with a reason, whether reaction I would beaccompanied by a decrease or increase in temperature.

(3)

(ii) At room temperature sulfur trioxide, SO3, is a solid. Deduce, with a reason, whether the

H

value would be more negative or less negative if SO3(s) instead of SO3(g) were


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formed in reaction II.(2)

(iii) Deduce the H value of this reaction:

S(s) +211 O2(g) SO3(g)

(1)

71. (i) Define the term average bond enthalpy.(3)

(ii) Explain why Br2 is not suitable as an example to illustrate the term average bond

enthalpy.(1)

(iii) Using values from Table 10 of the Data Booklet, calculate the enthalpy change for thefollowing reaction:

CH4(g) + Br2(g) CH3Br(g) + HBr(g)

(3)

(iv) Sketch an enthalpy level diagram for the reaction in part (iii).(2)

(v) Without carrying out a calculation, suggest, with a reason, how the enthalpy change for

the following reaction compares with that of the reaction in part (iii):

CH3Br(g) + Br2(g) CH2Br2(g) + HBr(g)

(2)

72. Throughout this question, use relevant information from the Data Booklet.

(a) Define the termstandard enthalpy change of formation, and illustrate your answer withan equation, including state symbols, for the formation of nitric acid.

(4)

(b) Propyne undergoes complete combustion as follows:

C3H4(g) + 4O2(g) 3CO2(g) + 2H2O(l)

Calculate the enthalpy change of this reaction, given the following additional values:

Hf of CO2(g) =394 kJ mol

1

Hf of H2O(l) =286 kJ mol

1

(4)

(c) Predict and explain whether the value ofS

for the reaction in part (b) would benegative, close to zero, or positive.

(3)

73. (a) Propyne reacts with hydrogen as follows:

C3H4(g) + 2H2(g) C3H8(g) H

=287 kJ

Calculate the standard entropy change of this reaction, given the following additionalinformation:

S of H2(g) = 131 J K1 mol1

(3)


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(b) Calculate the standard free energy change at 298 K, G, for the reaction in part (a). Use

your answer and relevant information from part (d). If you did not obtain an answer to

part (a), use S

=360 J K1

(this is not the correct value).(3)

74. (a) The lattice enthalpy of an ionic compound can be calculated using a Born-Haber cycle.

Using lithium fluoride as the example, construct a Born-Haber cycle, labeling the cyclewith the formulas and state symbols of the species present at each stage.

(6)

(b) Two values of the lattice enthalpies for each of the silver halides are quoted in the DataBooklet. Discuss the bonding in silver fluoride and in silver iodide, with reference tothese values.

(2)

75. But1ene gas, burns in oxygen to produce carbon dioxide and water vapour according to the

following equation.

C4H8 + 6O2 4CO2 + 4H2O

(a) Use the data below to calculate the value ofH for the combustion of but-1-ene.

Bond CC C=C CH O=O C=O OH

Average bond

enthalpy / kJ

mol1

348 612 412 496 743 463

(3)

(b) State and explain whether the reaction above is endothermic or exothermic.(1)

(Total 4 marks)

76. Calculate the enthalpy change, H4 for the reaction

C + 2H2 + 21 O2 CH3OH H4

using Hesss Law and the following information.

CH3OH + 211 O2 CO2 + 2H2O H1 = 676 kJ mol

1

C + O2 CO2 H2 = 394 kJ mol1

H2 + 21 O2 H2O H3 = 242 kJ mol

1

77. Hex-1-ene gas, C6H12, burns in oxygen to produce carbon dioxide and water vapour.

(a) Write an equation to represent this reaction.

(b) Use the data below to calculate the values ofHc and Sc

for the combustion of

hex-1-ene.

Substance O2(g) C6H12(g) CO2(g) H2O(g)

Standard enthalpy of

formation, Hf / kJ1 mol 0.0 43 394 242

Entropy, S / J K1 mol1 205 385 214 189

(i) Value ofHc (2)


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(ii) Value ofSc

(2)

(c) Calculate the standard free energy change for the combustion of hex-1-ene. (2)

(d) State and explain whether or not the combustion of hex-1-ene is spontaneous at 25C. (1)

78. Calculate the enthalpy change, H4 for the reaction

C + 2H2 + 21 O2 CH3OH H4

using Hesss Law, and the following information.

CH3OH + 211 O2 CO2 + 2H2O H1 = 676 kJ mol

1

C + O2 CO2 H2 = 394 kJ mol1

H2 + 21 O2 H2O H3 = 242 kJ mol

1

79. Methylamine can be manufactured by the following reaction.

CH3OH(g) + NH3(g) CH3NH2(g) + H2O(g)

(a) Define the term average bond enthalpy. (2)

(b) Use information from Table 10 of the Data Booklet to calculate the enthalpy change forthis reaction. (4)

80. Methylamine can be manufactured by the following reaction.

CH3OH(g) + NH3(g) CH3NH2(g) + H2O(g)

(a) Define the termstandard enthalpy change of formation. (2)

(b) The values of standard enthalpy changes of formation for some compounds are shown inthe table.

Compound Hf / kJ mol1

NH3(g) 46

H2O(g) 242

Predict, with a reason, whether the value ofHf for H2O(l) is less than, greater than, or

equal to, the value ofHf

for H2O(g). (2)

(c) Use information from the table in (b) and from Table 11 of the Data Booklet to calculatethe enthalpy change for the reaction used to manufacture methylamine. (3)

81. (a) Define the term average bond enthalpy. (2)

(b) Use the information from Table 10 in the Data Booklet to calculate the enthalpy change

for the complete combustion of but-1-ene according to the following equation

C4H8(g) 4CO2(g) + 4H2O(g) (3)

(c) Predict, giving a reason, how the enthalpy change for the complete combustion ofbut-2-ene would compare with that of but-1-ene based on average bond enthalpies.

(d) The enthalpy level diagram for a certain reaction is shown below.


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HR

enthalpy of

reactants

HP

enthalpy of

products

Time

Enthalpy

State and explain the relative stabilities of the reactants and products.(2)

82. (a) Define the termstandard enthalpy change of formation, Hf.

(2)

(b) (i) Use the information in the following table to calculate the enthalpy change for thecomplete combustion of but-1-ene according to the following equation.

C4H8(g) + 6O2(g) 4CO2(g) + 4H2O(g)

Compound C4H8(g) CO2(g) H2O(g)

Hf / kJ mol1 + 1 394 242

(3)

(ii) Deduce, giving a reason, whether the reactants or the products are more stable.

(2)

(iii) Predict, giving a reason, how the enthalpy change for the complete combustion of

but-2-ene would compare with that of but-1-ene based on average bond enthalpies.(1)

83. The reaction between ethene and hydrogen gas is exothermic.

(i) Write an equation for this reaction. (1)

(ii) Deduce the relative stabilities and energies of the reactants and products. (2)

(iii) Explain, by referring to the bonds in the molecules, why the reaction is exothermic. (2)

84. (i) Define the termstandard enthalpy change of formation,Hf. (2)

(ii) Construct a simple enthalpy cycle and calculate the value ofHf (C2H5OH(l)) given the

following data.

Compound Hf / kJ mol1 Hcomb/ kJ mol1H2O(l) 286

CO2(g) 394

C2H5OH(l) 1371

(5)


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85. (i) Define the term average bond enthalpy.(2)

(ii) The equation for the reaction of ethyne and hydrogen is:

C2H2(g) + 2H2(g) C2H6(g)

Use information from Table 10 of the Data Booklet to calculate the change in enthalpyfor the reaction.

(2)

(iii) State and explain the trend in the bond enthalpies of the CCl, CBr and CI bonds.(2)

86. Consider the following reaction:

N2(g) + 3H2(g) 2NH3(g)

(i) Suggest why this reaction is important for humanity. (1)

(ii) Using the average bond enthalpy values in Table 10 of the Data Booklet, calculate thestandard enthalpy change for this reaction. (4)

(iii) The absolute entropy values, S, at 238 K for N2(g), H2(g) and NH3(g) are 192, 131 and

193 J K1 mol1 respectively. Calculate S for the reaction and explain the sign ofS.(2)

(iv) Calculate G for the reaction at 238 K. State and explain whether the reaction is

spontaneous. (3)

(v) If ammonia was produced as a liquid and not as a gas, state and explain the effect this

would have on the value ofH

for the reaction. (2)

87. (i) Define the terms lattice enthalpy and electron affinity. (2)

(ii) Use the data in the following table and from the data booklet to construct the Born-Habercycle for sodium chloride, NaCl, and determine the lattice enthalpy of NaCl(s). (4)

Na(s) +2

1Cl2(g) NaCl(g) H

=411 kJ mol1

Na(s) Na(g) H= +108 kJ mol1

(iii) Describe the structure of sodium chloride. (2)

88.

Number ofmolecules

Ea Energy

The diagram shows the distribution of energy for the molecules in a sample of gas at a given

temperature, T1.

(a) In the diagramEa represents the activation energy for a reaction. Define this term.


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(b) On the diagram above draw another curve to show the energy distribution for the samegas at a higher temperature. Label the curve T2. (2)

(c) With reference to your diagram, state and explain what happens to the rate of a reactionwhen the temperature is increased. (2)

89. (a) Define the term average bond enthalpy, illustrating your answer with an equation formethane, CH4. (3)

(b) The equation for the reaction between methane and chlorine is

CH4(g) + Cl2(g) CH3Cl(g) + HCl(g)

Use the values from Table 10 of the Data Booklet to calculate the enthalpy change forthis reaction. (3)

(c) Explain why no reaction takes place between methane and chlorine at roomtemperature unless the reactants are sparked, exposed to UV light or heated. (2)

(d) Draw an enthalpy level diagram for this reaction.

90. The equation for the decomposition of calcium carbonate is given below.

CaCO3(s) CaO(s) + CO2(g)

At 500 K, Hfor this reaction is +177 kJ mol1 and Sis 161 J K

1 mol1.

(a) Explain why Hfor the reaction above cannot be described as Hf.

(b) State the meaning of the term S.

(c) Calculate the value ofG at 500 K and determine, giving a reason, whether or not thereaction will be spontaneous.

91. In aqueous solution, potassium hydroxide and hydrochloric acid react as follows.

KOH(aq) + HCl(aq) KCl(aq)+ H2O(l)

The data below is from an experiment to determine the enthalpy change of this reaction.

50.0 cm3 of a 0.500 mol dm3 solution of KOH was mixed rapidly in a glass beaker with

50.0 cm3 of a 0.500 mol dm3 solution of HCl.

Initial temperature of each solution = 19.6C

Final temperature of the mixture = 23.1C

(a) State, with a reason, whether the reaction is exothermic or endothermic. (1)

(b) Explain why the solutions were mixed rapidly. (1)

(c) Calculate the enthalpy change of this reaction in kJ mol1. Assume that the specific heat

capacity of the solution is the same as that of water. (4)

(d) Identify the major source of error in the experimental procedure described above.Explain how it could be minimized. (2)

(e) The experiment was repeated but with an HCl concentration of 0.510 mol dm3 instead


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of 0.500 mol dm3

. State and explain what the temperature change would be. (2)

92. The standard enthalpy change for the combustion of phenol, C6H5OH(s), is3050 kJ mol1

at 298 K.

(a) Write an equation for the complete combustion of phenol (1)

(b) The standard enthalpy changes of formation of carbon dioxide, CO2(g), and of water,

H2O(l), are394 kJ mol1 and286 kJ mol1 respectively.

Calculate the standard enthalpy change of formation of phenol, C6H5OH(s). (3)

(c) The standard entropy change of formation, S, of phenol, C6H5OH(s) at

298 K is385 J K1

mol1

. Calculate the standard free energy change of formation,

G, of phenol at 298 K. (3)

(d) Determine whether the reaction is spontaneous at 298 K, and give a reason. (2)

(e) Predict the effect, if any, of an increase in temperature on the spontaneity of this reaction.(2)

93. The data below is from an experiment used to measure the enthalpy change for the combustionof 1 mole of sucrose (common table sugar), C12H22O11(s). The time-temperature data was taken

from a data-logging software programme.

Mass of sample of sucrose, m = 0.4385 g

Heat capacity of the system, Csystem = 10.114 kJ K1

(a) Calculate T, for the water, surrounding the chamber in the calorimeter. (1)


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(b) Determine the amount, in moles, of sucrose. (1)

(c) (i) Calculate the enthalpy change for the combustion of 1 mole of sucrose. (1)

(ii) Using Table 12 of the Data Booklet, calculate the percentage experimental errorbased on the data used in this experiment. (1)

(d) A hypothesis is suggested that TNT, 2-methyl-1,3,5-trinitrobenzene, is a powerfulexplosive because it has:

a large enthalpy of combustion a high reaction rate a large volume of gas generated upon combustion

Use your answer in part (c)(i) and the following data to evaluate this hypothesis:

Equation for combustion Relativerate of

combustion

Enthalpy of

combustion

/ kJ mol1

Sucrose C12H22O11(s) + 12O2(g) 12CO2(g) + 11H2O(g) Low

TNT 2C7H5N3O6(s) 7CO(g) + 7C(s) + 5H2O(g) + 3N2(g) High 3406(3)

94. (a) Use the information from Table 10 of the Data Booklet to calculate the enthalpy changefor the complete combustion of but-1-ene, according to the following equation.

C4H8(g) + 6O2(g) 4CO2(g) + 4H2O(g)

(3)


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ANSWERS

95. D 96. C

97. B 98. D

99. D 100. D

101. D 102. B

103. A 104. A

105. C 106. B

107. B 108. A

109. B 110. B

111. C 112. B

113. C 114. D

115. C 116. B

117. A 118. A

119. D 120. D

121. A 122. D

123. C 124. B

125. A 126. C

127. C 128. A

129. D 130. C

131. A 132. C

133. D 134. A

135. B 136. C

137. C 138. A

139. D 140. C

141. A 142. C

143. B 144. C

145. D 146. B

147. A 148. D

149. B 150. C

151. C 152. B

153. B 154. C

155. B 156. D

157. C(s) + 2F2(g) CF4(g) H1 =680 kJ;

4F(g) 2F2(g) H2 = 2(158) kJ;

C(g) C(s) H3 =715 kJ;

Accept reverse equations with +H values.

C(g) + 4F(g) CF4(g) H=1711 kJ,

so average bond enthalpy =

4

1711

=428 kJ mol1; 4

Accept + orsign.


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Lots of ways to do this! The correct answer is very differentfrom the value in the Data Booklet, so award[4]for finalanswer with/without sign units not needed, but deduct[1]ifincorrect units. Accept answer in range of 427 to 428 withoutpenalty for sig figs.

If final answer is not correct use following;

Award[1]for evidence of cycle or enthalpy diagram or adding

of equations.Award[1]for 2F2 (g) 4F(g) 2158 seen.

Award[1]for dividing 1711 or other value by 4.[4]

158. (G

= HTS)

as Tincreases,TS

becomes larger/more positive;G increases/becomes more positive/less negative;process becomes less spontaneous/reverse reaction favoured; 3

[3]

159. a reaction is spontaneous when G is negative/non-spontaneous when G is positive;

at high T, Gis negative;

(because) TS

is greater than H;

at low T, Gis positive because TSis smaller than H/OWTTE; 4[4]

160. (i) selection of all the correct bonds or values from Data Booklet;H= (NN) + 3(HH)6(NH) / 944 + 3(436)6(388);=76 (kJ); 3

Allow ECF for one error (wrong bond energy/wrongcoefficient/reverse reaction) but not for two errors(so611,857, +76, +1088 all score 2 out of 3).

(ii) negative;

decrease in the number of gas molecules/OWTTE; 2

(iii) G = HTSG =76.0300 (0.0627); 3

Award[1]for 300 K.

Award[1]for conversion of units J to kJ or vice versa.Allow ECF from (i) fromH.Allow ECF from (ii) for sign ofS.

=57.2 (kJ mol1

) is spontaneous/or non-spontaneous if positive valueobtained; [3 max]

[8]

161. a reaction is spontaneous when G

is negative;

at high T, G

is negative;TS is larger/greater than H;

at low T, G

is positive becauseTS

is smaller than H/OWTTE; 4

[4]

162. (i) H= (sum of energies of bonds broken)(sum of energies of bonds formed);

Can be implied by working.

Correct substitution of values and numbers of bonds broken;

Correct substitution of values and numbers of bonds made;

(H= (NN) + 3(HH)6(NH) = 944 + 3(436)6(388) =)76 (kJ);4

Allow ECF.Do not penalize for SF or units.

(ii) S

= (sum of entropies of products)(sum of entropies of reactants); 3


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Can be implied by working.

(= 2192(193 + 3131) =)202(J K1 mol1);

four molecules make two molecules/fewer molecules of gas;

(iii) (G=HTS=76.0300(0.202)) =15.4 (kJ mol 1); 1Do not penalize for SF.

(iv) H

becomes more negative; 2heat released when gas liquid;

[10]

163. enthalpy change associated with the formation of one mole of acompound/substance; from its elements;in their standard states/under standard conditions;

2C(s) + 3H2(g) + 21 O2(g) C2H5OH(l); 5

Award[1]for formulas and coefficients, [1]for state symbols.

[5]

164. (a) (i) standard enthalpy (change) of reaction;(temperature) increase;

reaction is exothermic/sign ofH is negative; 3

(ii) more (negative);heat given out when gas changes to solid/solid has less enthalpy thangas/OWTTE; 2

(iii) 389 kJ; 1[6]

165. (i) the energy needed to break one bond;(in a molecule in the) gaseous state;

value averaged using those from similar compounds; 3

(ii) it is an element/no other species with just a Br-Br bond/OWTTE; 1

(iii) (sum bonds broken =) 412 + 193 = 605;

(sum bonds formed =) 276 + 366 = 642;(H

=)37 kJ; 3

Award[3]for correct final answer.

Award[2]for + 37.

Accept answer based on breaking and making extra C-H bonds.

(iv)

Enthalpy

CH4 + Br2

CH3Br + HBr

;

2Award[1]for enthalpy label and two horizontal lines, [1]forreactants higher than products.

ECF from sign in (iii), ignore any higher energy level involvingatoms.

(v) (about) the same/similar;same (number and type of) bonds being broken and formed; 2

[11]

166. (a) the enthalpy/energy/heat change for the formation of one mole of acompound/substance from its elements;

in their standard states/under standard conditions/at 298 K and 1 atm;

;)l(HNO(g)O1(g)N(g)H 3221

221

221 4


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Award[1]for correctly balanced equation, [1]for all statesymbols correct.

Do not award equation mark if 2HNO3 formed.

(b) Hr= Hf

(products) Hf

(reactants)/suitable cycle;

= 3( 394) + 2( 286) 185;Award[1]for correct coefficients of CO2 and H2O values, [1]

for correct value for C3H4 from Data Booklet.

= 1939 or1940 kJ; 4Ignore units.


Award[3]for +1939 or1569.

(c) negative;

decrease in disorder/increase in order;

5 mol of gas 3 mol of gas/reduction in number of gas moles; 3Award[1]for answer of close to zero based on use of H2O(g).

[11]

167. (a) S= S (products) S (reactants)/suitable cycle;

= 270 248 2131;

= 240 (J K1); 3

Units not needed for mark, but penalize incorrect units.


(b) G

= 287 (2980.240);Award[1]for correct substitution of values and[1]for

conversion of units.

= 215 kJ; 3Units needed for mark.

Apply ECF from 360 kJ or incorrect answer from (a).

[6]

168. (a) 6

LiF(s)

122

Li(s) F (g)+

122

Li(g) F (g)+

Li (g) F (g)+ -

+

Li (g) e F(g)+ -+ +

122

Li (g) e F (g)+

-+ +

Award[6]for completely correct cycle, with endothermic

processes in any order.Deduct[1]for each line in which species symbol and/or state

symbol is incorrect or missing.


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Penalize missing electrons once only.

(b) bonding in AgF more ionic than in AgI/bonding in AgI more covalent thanin AgF;

Accept AgF is ionic and AgI is covalent.

values closer/in better agreement in AgF/big(ger) difference in values forAgI/OWTTE; 2

[8]

169. (a) (Amount of energy required to break bonds of reactants)

8412 + 2348 + 612 + 6496/7580 (kJ mol1);

(Amount of energy released during bond formation)

42743 + 42463/9648 (kJ mol1);

H= 2068 (kJ or kJ mol1); 3

ECF from above answers.

Correct answer scores [3].

Award[2]for (+)2068.

If any other units apply 1(U), but only once per paper.(b) exothermic andH

is negative/energy is released; 1

Apply ECF to sign of answer in part (a).

Do not mark if no answer to (a).

[4]

170. 1H1/676;

1H2/394;

2H3/484;

H4 = 202 (kJ mol1 ); 4

Accept alternative methods.

Correct answers score [4].

Award[3]for (+)202 or (+)40 (kJ/kJ mol1).

1(U) if units incorrect (ignore if absent).

[4]

171. (a) C6H12 + 9O2 6CO2 + 6H2O; 1

(b) (i) (H = Hf

productsHf

reactants)

H

= (6394 + 6242) (43);

Hc = 3773/3.8103 (kJ mol1); 2

Accept 2, 3 or 4 sig. fig..

Award[1]for + 3773/+ 3.8 103 (kJ mol1).

Allow ECF from (a) only if coefficients used.

(ii) S

= (Sp

Sr

) = (6189 + 6214) (385 + 9205);

S =188 (J K1 mol1 ); 2Accept only 3 sig. fig..

Award[1]for188.

Allow ECF from (a) only if coefficients used.

(c) (G

c = H

c TS

c) = 3800 (2980.188);

= 3900 kJ mol1. 2

Accept3800 to 3900.

Accept 2, 3 or 4 sig. fig.

Allow ECF from (b).


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Units needed for second mark.

(d) spontaneous and G negative; 1Allow ECF from (c).

[8]

172. 1H1/676;

1H2/ 394;

2H3/ 484;

H4 = 202 (kJ mol1); 4

Accept alternative methods.

Correct answers score [4].

Award[3]for (+)202 or (+)40 (kJ/kJ mol1

).

[4]

173. (a) energy needed to break (1 mol of) a bond in a gaseous molecule;averaged over similar compounds; 2

(b) bonds broken identified as CO and NH;

bonds formed identified as CN and OH;

H= 748 768 (kJ);

= 20 kJ/kJ mol1

(units needed for this mark); 4If wrong bonds identified apply ECF to 3rd and 4th marks.

Accept answer based on breaking and making all bonds.


Award max [3]if only one bond missed.

Answer of 20 or +20 kJ (mol1

) scores [3].

174. (a) enthalpy/energy change for the formation of 1 mol of a compound from

its elements;Do not acceptheatneeded to form 1 mol

in their standard states/under standard conditions/at 298 K and 1 atm; 2

(b) greater value/more negative value;

energy given out when steam condenses/turns to water; 2

(c) H

= Hf

(products) Hf

(reactants)/suitable cycle;

= (28242)(20146);

= 23 kJ/kJ mol1; 3Units needed for 3rd mark.

Correct final answer scores [3].23 or +23 kJ/kJ mol

1scores [2].

If239 used instead of201 for CH3OH, award[2]for +15 kJ.

[7]

175. (a) amount of energy needed to break one mole of (covalent) bonds;in the gaseous state;average calculated from a range of compounds; 2

Award[1]each for any two points above.

(b) bonds broken: 161 + 2348 + 8412 + 6496/7580 kJ mol1;

bonds made: 8743 + 8463/9648 kJ mol1;

(bonds broken bonds made =) H= 2068(kJ mol1); 3

Award[3]for the correct answer.


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Allow full ECF1 mistake equals 1 penalty.

Allow kJ but not other wrong units.

(c) same/equal, because the same bonds are being broken and formed; 1

(d) products more stable than reactants;

bonds are stronger in products than reactants/HP < HR/enthalpy/stored

energy of products less than reactants; 2[8]

176. (a) the enthalpy change when one mole of compound is formed from its elements

in their (standard state);at (standard conditions of) 298 K/25C and 101 325 Pa/1 atm; 2

(b) (i) HP = (4242 + 4394) kJ mol1;

HR = 1 kJ mol1;

H

= (H

pH

R) = 2545 /2.55103/ 2550 (kJ mol

1); 3

Allow ECF.

(ii) products more stable than reactants;

bonds are stronger in products than reactants/Hp


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28

Hcomb

Hf (C2H5OH(l));

2Hf

(CO2(g)) and 3Hf

(H2O(l));

(Hf

(C2H5OH(l)) = (2Hf

(CO2(g)) + 3Hf

(H2O(l)) Hcomb

= 2(394) + 3(286) + 1371;

= 275 kJ mol1; 5If values are substituted for symbols in the enthalpy cycle

diagram to give correct answer, award last[2]marks.

If no enthalpy cycle drawn but equation written and Hesss

Law applied or calculated as follows, then [3 max]

(Hr= Hf(products) Hf(reactants))

1371 = (3942) + (2863) Hf(ethanol);

Hf(ethanol) = 788 858 + 1371;

= 275(kJ mol1);

Award[2]for correct answer without enthalpy cycle andwithout working and[1]for 275 or + 275.

[7]

179. (i) energy required to break (a mole of) bonds in the gaseous state

/energy given out when (a mole of) bonds are made in thegaseous state;average value from a number of similar compounds; 2

(ii) (H

reaction = (BEbreakBEmake))

= [(837) + 2(436)] [(348 + 4(412)];

= 287(kJ/kJ mol1); 2

Award[1 max]for 287 or + 287.

(iii) (BE): CCl > CBr > CI/CX bond becomes weaker;halogen size/radius increases/bonding electrons further away from

the nucleus/bonds become longer; 2[6]

180. (i) fertilizers/increasing crop yields;

production of explosives for mining; 1 max

(ii) H= (sum of energies of bonds broken)(sum of energies of bonds formed);Can be implied by working.

correct substitution of values and numbers of bonds broken;correct substitution of values and numbers of bonds made;

(H= (NN) + 3(HH)6(NH) = 944 + 3(436)6(388) =)76.0 (kJ); 4Allow ECF.

Do not penalize for sig. fig. or units.Award[4]for correct final answer.

(iii) (S[2193][192 + 3131]) =199 (J K

1mol

1); 2

Allow ECF.four gaseous molecules generating two gaseousmolecules/fewer molecules of gas;

(iv) (G

= HTS

=76.0298(0.199)) =16.7 (kJ);

Spontaneous;

G is negative; 3Do not penalize for SF.

(v) heat released when gas liquid;

H

becomes more negative; 2


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[12]

181. (i) lattice enthalpy for a particular ionic compound is defined as Hfor the

process, MX(s) M+(g) + X

(g);

Accept definition for exothermic process

electron affinity is the energy change that occurs when an electron is addedto a gaseous atom or ion; 2

(ii)

Na(s)

+108 kJ mol1

+

Na(g)

Na (g)+ +

H = 411 kJ mol1

+494 kJ mol1

Cl (g)1 2 NaCl(s)

+121 kJ mol

364 kJ mol

Cl(g)

Cl (g)

f

1

1

2

lattice enthalpy =[(411)(+108)(+494)(+121)(364)]

= 770 (kJ mol1)

Award[2]for all correct formulas in correct positions on cyclediagram.

1 incorrect or missing label award[1].Award[1]for all correct values in correct positions on cycle

diagram.

calculation of lattice enthalpy of NaCl(s) = 770 (kJ mol1); 4

Allow ECF.Accept alternative method e.g. energy level diagram.

(iii) lattice/network/regular structure;each chloride ion is surrounded by six sodium ions and each sodium ion issurrounded by six chloride ions/6:6 coordination; 2

[8]

182. (a) activation energy = minimum energy required for a reaction to occur; 1

(b) curve moved to the right;peak lower, 2

Deduct[1]if shaded area smaller at T2 or if T2 line touches the

x-axis

(c) rate increased;as more molecules with energy Ea; 2

[5]

183. (a) energy for the conversion of a gaseous molecule into (gaseous) atoms;(average values) obtained from a number of similar bonds/compounds/OWTTE;CH4(g) C(g) + 4H(g); 3

State symbols needed.

(b) (bond breaking) = 1890/654;(bond formation) = 2005/769;

enthalpy =115(kJ mol1) 3Allow ECF from bond breaking and forming.


Penalize [1]for correct answer with wrong sign.


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(c) molecules have insufficient energy to react (at room temperature)/wrong collision geometry/unsuccessful collisions;extra energy needed to overcome the activation energy/Ea for the reaction; 2

(d)

energy reactants

reaction path

products

Ea

exothermic shown;

activation energy/Ea shown; 2

Allow ECF from (b).

[10]

184. (a) (cannot be as) conditions are not standard/at 500 K/OWTTE;(cannot be f as) not formation from elements/is decomposition/OWTTE; 2

(b) change in entropy/degree of (dis)order (of system); 1

(c) G = 177000(500161) = +96500;reaction is not spontaneous;

G is positive; 3Allow ECF from calculation for last two marks.

[6]

185. (a) exothermic because temperature rises/heat is released; 1

(b) to make any heat loss as small as possible/so that all the heat will begiven out very quickly; 1

Do not accept to produce a faster reaction.

(c) heat released = massspecific heat capacitytemp increase/q = mcT=/1004.183.5;= 1463 J/1.463 kJ; (allow 1.47 kJ if specific heat = 4.2)amount of KOH/HCl used = 0.5000.050 = 0.025 mol;

H= (1.4630.025) =58.5 (kJ mol1

); (minus sign needed for mark) 4Use ECF for values of q and amount used.


Final answer of 58.5 or +58.5 scores [3].

Accept 2,3 or 4 significant figures.

(d) heat loss (to the surroundings);insulate the reaction vessel/use a lid/draw a temperature versus time graph; 2

(e) 3.5C/temperature change would be the same;amount of base reacted would be the same/excess acid would not react/KOH is the limiting reagent; 2

[10]

186. (a) C6H5OH + 7O2 6CO2 + 3H2O; 1

Ignore state symbols.

(b) Hr=Hf

productsHf reactants;

3050 = (6(394) +3 (286)(Hf

phenol + O));


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Hf

phenol =172 kJ mol1

; 3


Apply1 (U) if appropriate.

Award[2 max]forHf

phenol = +172 kJ mol1

.

(c) appropriate conversion of units;G =172298(0.385)

=57.3 kJ mol1/57 300 J mol1; 3Award[3]for correct final answer.

Accept answers in range57.0 to57.3 kJ mol1.Accept 3 sig. fig. only.

Allow ECF from (b).Apply1 (U) if appropriate.

(d) spontaneous;since G is negative;

Allow ECF from (c). 2

(e) reaction becomes less spontaneous;G becomes less negative/more positive;

Accept a suitable calculation.

Allow ECF from (c). 2

187. (a) T= 23.7023.03 = 0.67 (C/K); 1

(b)

1molg342.34

g4385.0n = 1.28110

3; 1

(c) (i) Hc = (CT)/n =mol)10281.1(

K)]67.0)(KkJ114.10[(3

1

=5.3103 kJ mol1; 1

Use ECF for values ofT and n.

(ii) Percentage experimental error = 100)106.5(

)106.5()103.5(3

33

= 5.4%; 1

Use ECF for values of Hc.

(d) enthalpy change of combustion of sucrose > TNT, and therefore not important;rate of reaction for TNT is greater than that of sucrose, so this is valid;amount of gas generated (in mol) for sucrose > than that of TNT

(according to the given equation), so this is not important; 3[7]

188. (a) The amount of energy needed to break 1 mole of (covalent) bonds;in the gaseous state;average calculated from a range of compounds; 2 max

Award[1]each for any two points above.

(b) Bonds broken

(612) + (2348) + (8412) + (6496)/7580 (kJ mol1

);Bonds made

(8743) + (8463) / 9648 (kJ mol1);

H=2068 (kJ mol1

); 3Award [3] for the correct answer.Allow full ECF.Allow kJ but no other incorrect units.


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Even if the first two marks are lost, the candidate can score [1]

for a clear correct subtraction forH.

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Energetics Q + MS