FIRST YEAR - IPE CHEMISTRY - FIITJEE Hyderabad YEAR - IPE CHEMISTRY `KUKATPALLY CENTRE Total No. of Questions - 21 Reg. Total No. of Printed Pages - 2 No. Paper - I CHEMISTRY IPE BOARD

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FIRST YEAR - IPE CHEMISTRY

` KUKATPALLY CENTREKUKATPALLY CENTREKUKATPALLY CENTREKUKATPALLY CENTRE

Total No. of Questions - 21 Reg .

Total No. of Printed Pages - 2 No.

Paper - I

CHEMISTRY

IPE BOARD MODEL PAPER FOR THE YEAR MARCH 2014 (English Version)

Time : 3 Hours] [Max. Marks : 60

SECTION - A 10 × 2 = 20 M

I. Very Short Answer Type questions:

1. Define COD, BOD

2. Define Greeen House effect . Which gases are the cause for it?

3. State Dalton’s law of partial pressures.

4. Write the properties of washing soda.

5. Write the important uses of quick lime

6. How many number of moles of glucose are present in 540 gms of glucose?

7. Give the use of 2CO in photosynthesis.

8. What is Homogenous equilibrium? Give one example.

9. Name any two man-made silicates?

10. Write the structural formula of the given compounds.

a) 3,4,4,5-tetramethyl heptane b) 2-methyl 1-butene

SECTION – B 6 × 4 = 24 M

II. Short Answer Type questions: (i) Attempt any six questions (ii) Each question carries four marks

11. State and explain the Hess’s law of constant heat summation with example.

12. Define Graham’s law of diffusion. Calculate kinetic energy of moles of nitrogen at 27 C° .



13. Balance the following equation in basic medium by ion-electron method.

4 2 2MnO I MnO I− −+ → +

14. What is conjugate acid-base pair? Write the conjugate acid and conjugate base of each of the

following?

a) OH− b) 3HCO −

15. Explain the following with suitable examples.

a) Electron-deficient hydrides b) Electron-precise hydrides.

16. Give two methods of preparation of Diborane.

17. How do you get Benzene from Acetylene. Explain the halogenation and alkylation of Benzene.

18. Describe two methods of preparation of Ethylene. Give the equation for the reactions of ethylene

with the following:

a) Ozone b) Cold and alk. 4KMnO

SECTION – C 2 × 8 = 16 M

III. Long Answer Type questions: (i) Attempt any two questions (ii) Each question carries eight marks

19. What are Quantum numbers? Explain the significance of these quantum numbers.

20. What is Periodicity? How the following properties vary in a Group and in a Period? Explain.

a) Atomic radius b) IE c) EN

21. Define Hybridisation

a) Explain the structure of 6SF by hybridization

b) Calculate the bond orders of 2 2,N O molecules.






Paper - I

CHEMISTRY

IPE BOARD MODEL PAPER FOR THE YEAR MAY 2014 (English Version)


SECTION - A 10 × 2 = 20 M


1. What are greenhouse gases? Give examples.

2. Why are IA group elements called as alkali metals?

3. Find the RMS velocity of 2CO gas at 27 C° ?

4. What is chemical oxygen demand (COD).

5. How many number of 3CaCO moles are present in 200 gms of 3CaCO ?

6. Derive the PK and CK relations for the reaction.

( ) ( ) ( )5 3 2g g gPCl PCl Cl+��⇀↽��

7. What is plaster of paris? Mention its uses.

8. 4CCl is not dissolved in water, but 4SiCl dissolves. Why? Give reasons.

9. Write the hybridization of carbon in the following:

a) 2CO b) Diamond c) Graphite d) Fullerenes

10. Draw the cis-trans isomers for the following compounds.

a) CHCl CHCl= b) 2 5 3 3 2 5C H CH C CCH C H=

SECTION – B 6 × 4 = 24 M


11. State Graham’s law of diffusion. Write any two of its applications.

12. Balance the following equations in an acid medium by the ion-electron method or the half reaction

method.

2 3 22 7 2 4Cr O SO Cr SO− −+ → +



13. Define the following terms:

a) Enthalpy b) Entropy

14. What is HP ? Find the HP of a 0.1 M HCl solution.

15. What is temporary and permanent hardness of water? Mention which ions cause the hardness of

water.

16. What are electron deficient compounds? Explain why 3BF acts as a Lewis acid.

17. Complete the following reaction and name the products A, B and C.

2 4 32 . 2 323 333

Conc H SO HNOH O Hot Cu tube

KCaC A B C+

−→ → →

18. Write notes on the following:

a) Distillation b) Chromatography

SECTION – C 2 × 8 = 16 M

III. Long Answer Type questions: (i) Attempt any two questions (ii) Each question carries eight marks

19. Write the important postulates of Bohr’s atomic model and explain how spectral lines are formed in

the hydrogen spectrum with a neat diagram.

20. What is periodicity? Explain the following periodic trends.

a) atomic size b) ionization energy c) electronegativity

21. Give the molecular orbital energy diagram of 2N and 2O . Write the bond order of 2N and 2O .






Paper - I

CHEMISTRY



SECTION - A 10 × 2 = 20 M


1. Calculate the RMS speed of nitrogen molecules at 27 C° ?

2. What is disproportionation reaction? Give example.

3. Calculate the pH of 0.05M ( )2

Ba OH solution.

4. Give the biological importance of magnesium and calcium.

5. Give the reactions that take place at anode and cathode in Castner - Kellner process.

6. Graphite is a good conductor of electricity. Why?

7. What is allotropy? Name two crystalline allotropes of carbon.

8. Define the terms COD and BOD?

9. What are the harmful effects of acid rains?

10. Give the structural formulae of the following compounds

a) 2,3-dimethyl butane b) 2-methyl but-1-ene

SECTION – B 6 × 4 = 24 M


11. Write any four postulates of Kinetic Molecular Theory of gases.

12. Balance the following redox equation in acidic medium by ion-electron method

2 24 2 4 2MnO C O Mn CO− − ++ → +

13. State Hess’s law of constant heat summation. Explain with one example.

14. Derive the relation between Kp and Kc for the equilibrium reaction.

( ) ( ) ( )2 2 33 2

g g gN H NH+ ⇌



15. Explain electrolytic method of preparation of hydrogen peroxide.

16. Explain the structure of diborane on the basis of VBT.

17. Explain (a) position isomerism and (b) functional group isomerism with one example for each of

them.

18. Explain (a) Wurtz reaction and (b) Friedel – Craft’s reaction with one example for each of them.

SECTION – C 2 × 8 = 16 M

III. Long Answer Type questions: (i) Attempt any two questions (ii) Each question carries eight marks 19. What are quantum numbers? Explain the significance of the four quantum numbers associated

with an electron.

20. Define first and second ionisation potentials. Why the second ionisation potential of an element is

always greater than first ionisation potential? Explain any four factors that affect the ionisation

potential of an element.

21. (a) Explain 3sp d hybridisation with one example.

(b) Explain molecular orbital theory of oxygen molecule. Calculate it’s bond order and explain it’s

magnetic property.






Paper - I

CHEMISTRY

IPE BOARD MODEL PAPER FOR THE YEAR MAY 2013 (English Version)


SECTION - A 10 × 2 = 20 M


1. Write the biological importance of Mg and Ca.

2. Write any two uses of caustic soda.

3. Write two crystalline allotropes of carbon and mention hybridization present in them.

4. Why Diamond is hard?

5. What is Green House Effect?

6. What are the effects of Acid Rains?

7. Calculate kinetic energy of 3 moles of 2CO gas at 27 C°

8. The empirical formula of a compound is 2CH O Its molecular weight is 90. Find the molecular

formula of the compound.

9. Concentration of hydrogen ion is 33.8 10 M−× . What is its pH?

10. Write IUPAC names of the following:

CH3

CH3

CH3

CH

CH3

CH2CH3

CH3

CH3

CH3

CH2COOH

(a) (b)

SECTION – B 6 × 4 = 24 M


11. Derive Charle’s law and Graham’s law of diffusion from kinetic gas equation.

12. Balance the following Redox reaction by ion electron method or half cell reaction method.

24 2 2

acid

mediumSO Br SO Br− −+ → +



13. State and explain Hess’s law of constant heat summation. Give example.

14. Derive the relation between PK and CK for the equilibrium reaction.

( ) ( ) ( )2 2 32 2g g g

SO O SO+ ��⇀↽��

15. What is hardness of water? Write Calgon’s method for the removal of permanent hardness of

water.

16. Explain the structure of Diborane.

17. Write two methods of preparation of Ethylene. Give the equations.

18. How the following are obtained from Benzene?

a) Nitro Benzene b) Methyl Benzene

SECTION – C 2 × 8 = 16 M

III. Long Answer Type questions: (i) Attempt any two questions (ii) Each question carries eight marks 19. What are Quantum numbers? Explain the significance of Quantum numbers.

20. What is first and second ionization potential? Why 2 1I I> ?

Explain four factors influencing ionization potential.

21. a) Explain coordination covalent bond with example.

b) What is hybridization? Explain 3sp d hybridization with example.






Paper - I

CHEMISTRY



SECTION - A 10 × 2 = 20 M


1. Define ‘receptor’ and ‘sink’.

2. Which oxides cause acid rain? What is its pH value?

3. Write about the biological importance of calcium.

4. The empirical formula of a compound is 2CH O . Its molecular weight is 90. Calculate the molecular

formula of the compound.

5. What is allotropy? Give the crystalline allotropes of carbon.

6. Calculate kinetic energy of 5 moles of nitrogen at 27 C° .

7. Why is carbon monoxide poisonous?

8. Calculate the pH of 0.05 M NaOH solution.

9. Why are alkali metals not found in a free state in nature.

10. Write the structural formulae of the following compounds:

a) Trchloroethanoic acid b) Neo-pentane

SECTION – B 6 × 4 = 24 M


11. Write any four postulates of the kinetic molecular theory of gases.

12. Calculate the molarity of sodium carbonate in a solution prepared by dissolving 5.3g in enough

water to form 250 ml of the solution.

13. State Hess law of constant heat summation. Explain with one example.



14. Derive the relation between PK and CK for the equilibrium reaction

( ) ( ) ( )2 2 33 2g g g

N H NH+ ��⇀↽��

15. Write few lines on the utility of hydrogen as a fuel.

16. What is borax? Explain the borax bead test with a suitable example.

17. Explain Wurtz reaction and Friedel Crafts alkylation with one example for each.

18. Write about position isomerism and functional group isomerism.

SECTION – C 2 × 8 = 16 M

III. Long Answer Type questions: (i) Attempt any two questions (ii) Each question carries eight marks 19. What are the postulates of Bohr’s model of a hydrogen atom? Write any two limitations of Bohr’s

model of an atom.

20. Define first ionization energy and second ionization energy. Why is the second ionization energy

greater than the first ionization energy for a given atom? Discuss any four factors that affect the

ionization energy of an element.

21. What do you understand by hybridization? Explain the different types of hybridizations involving

' 's and ' 'p orbitals.



VERY SHORT ANSWER QUESTIONS MAY 2011

SECTION - A

1. Write any two effects of polluted water. A. Bad effects of polluted water: not useful for drinking; destruction of aquatic life; causes cholera, Jaundice,

diarrhoea. 2. Write the IUPAC name of the organic compound giv en below.

A.

3-Ethyl-4-Methyl Hexane

3. Calculate kinetic energy of 2 moles of

2O gas at 27 C° (R = 2 cal/K ).

A. 3nRT 3 2 2 300

K.E. 1800 cal.2 2

× × ×= = =

4. What are the effects of Acid Rains? A. Effects of Acid Rains: Change in pH of soil effects soil fertility; destruction of aquatic life, destruction of marble

momuments. 5. Name the products A and B formed in the followin g reactions:

alkaline KMnO4

3 6 Agl 25 C2 CH I 6 Ag A

∆− °

+ → → B.

A. COOHalk.

3 6 AgI KMnO(A) 4 COOH(B)

2CHI 6Ag CH CH |∆−

+ → ≡ →

A=Acetylene; B=oxalic Acid 6. What is shielding effect? How does it effect the IP values? A. Shielding Effect: Lowering of nuclear attraction on valence electrons. Increase in shielding effect causes;

Decrease in I.P. (1

I.PS.E.

α ).

7. In how many stages plaster of paris sets to a ha rd mass? Write equation. A. Plaster of Paris sets in two stages

setting Hardening

4 2 2 4 2stage stageorthor hombic monoclinic

1 3CaSO H O H O CaSO 2H O Gypsom Gypsum

2 2⋅ + → ⋅ →

8. Calculate the oxidation numbers of Mn in 4

MnO− ion and Nitrogen in 3

NO− ion.

A. In 4

MnO− O.N of Mn 7= , in 3

NO− 0.N of N 5= + .

9. How heavy water reacts with calcium carbide? A. Reaction of

2D O with calcium carbide: ( ) ( )22 2 2 2

CaC 2D O Ca OD C D Heavy Acetylene+ → + ↑

10. What type of chemical bond will be formed betwe en K and Br atoms. If electronegativity of K is 0.8 and

Br is 2.8? A. Between K & Br ionic bond is formed because E.N diff > 1.7.



MARCH 2011

SECTION-A 1. Define Most Probable Velocity. A. Velocity possessed by maximum number of molecules is called most probable

velocityP

2RT 2PVC 2p d

M M= = = .

2. What is cause of Permanent hardness of water?

A. Permanent Hardness is due to presence of 24

SO− , Cl− of 2Mg+ , 2Ca+ ions.

3. How does Graphite acts as a lubricant? A. In graphite adjacent hexagonal sheets are held together by weak van der waal forces and can easily slide over

each other on application of pressure. So it acts as lubricant. 4. Calculate the Oxidation number of Carbon in

12 22 11C H O and

2CO .

A. In 12 22 11

C H O 0.N of C O= . In 2

CO 0.N of C 4= + .

5. Name the crystalline allotropes of Carbon and menti on the hybridization in them.

A. Carbon has two crystalline allotropes. Diamond – Carbon is 3sp , Graphite – Carbon is 2sp . 6. Define Receptor and Sink A. Receptor is the medium which is effected by pollutant ex. Marble monument receptor for acid rain. Sink is the

medium that reacts with pollutant ex. Plant is sink for 2

CO .

7. What are the effects of Acid rains? A. Effects of Acid rains: ref Q. 4 of May 2011. 8. Why are the carbides of Be and Al called methanides? A. Carbides of Be , Al on reaction with

2H O liberate

4CH gas. So they are called methanides.

( )22 2 4Be C H O Be OH CH+ → +

( )34 3 2 4Al C H O Al OH CH+ → +

9. What is Position isomerism? Give one example. A. Structural Isomerism that arises due to difference in position of functional group or substituent on carbon chain

ex. 1-propanol, 2-propanol. 10. Write the IUPAC names for the following compounds.

a)

CH3 C

CH3

CH3

CH

CH3

CH2 CH3

b)

CH3 C

CH3

CH3

CH2 COOH

A.

CH3 CCH3

CH3

CH

CH3

CH2 CH3

12 43 5

2,2,3-trimethyl pentane

CH3 CCH3

CH3

CH2 COOH1234

3,3-dimethyl butanoic acid



JUNE 2010

SECTION – A 1. State Graham’s law. A. Graham’s Law: Rate of diffusion of a gas at constant T, P is inversely proportional to square root of density or

vap. Density or Mol. wt. of gas. 1 1 1

rd vd M

α α α . For two given gases 1 2 2 2

2 1 1 1

r M d VD

r M d VD= = =

2. Give two uses of heavy water . A. Uses of

2D O :

(i) As moderator of neutrons in nuclear reactors. (ii) preparation of deuterium

(iii) as tracer to study the reaction mechanism and structures of 3 3

H PO , 3 2

H PO

3. How many moles of glucose are present in 540 gms of glucose?

A. weight

No. of moles = GMW

. No. of moles in 540gm of Glucose =540

3180

=

4. What is a diagonal relationship? Write an example. A. Diagonal Relationship: Similarity in properties of 1st element of a group with 2nd element of the next group is

called diagonal relationship ex. Li, Mg & B, Si are diagonal pairs. 5. Give equations for the formation of caustic soda fr om NaCl .

A. Preparation of NaOH by electrolysis of Nacl (aq). Reactions: 2NaCl 2Na 2Cl+ −→ +

22Cl Cl 2e(Anode)− → + ; ( )2 2

2H O 2e 2OH H cathode+ → + ; 2Na 2OH 2NaOH+ + → .

6. What is the biological importance of 2Mg+ and 2Ca+ ions?

A. Biological importance of 2Mg+ & 2Ca+ : 2Mg+ is present in animal cells and chlorophyll of plants, 2Ca+ is essential for blood clotting, muscular contraction, Heart beating, formation of bones.

7. Explain the Nalgonda defluoridation technique. A. Nalgonda defluoridation Technique: Fluoride ions of water are precipitated as complex calcium aluminium

fluoride by addition of bleaching powder, lime and alum in the same order. 8. What is greenhouse effect? A. Green House Effect: Warming up of Earth surface due to green house gases

2CO , CFC,

4CH ,

3O etc. is

known as Green House effect. 9. Name the functional group isomers of the molecular formula

3 6C H O .

A. Functional isomers with 3 6

C H O M.F.” 3 3

CH O CH− − dimethyl ether and 3 2

CH CH CHO− − propanal

are functional isomers with M.F. 3 6

C H O.

10. Give an example for the Wurtz’s reaction . A. Wurtz Reaction: Alkyl halide (Rx) on treatment with Na/dry ether produces alkane with double the number of

carbons. This reaction is called Wurtz Reaction. Ex: dry ether

3 3 3 3CH I 2Na I CH CH CH 2NaI− + + − → − + .



MARCH 2010

SECTION – A

1. What are the co-ordination numbers of NaCl and CsCl crystals.

A. Coordination number of Na+ or Cl− in NaCl is six (fcc)

Coordination number of Cs+ or Cl− in CsCl is eight (bcc) 2. What is the effect of Hydrogen bonding on boiling p oints? A. Effect of H-bonding on boiling points. Due to intermolecular H-bonding molecules get associated so B.pt

increases. Ex. 2

H O has more B.pt than 2

H S. Due to intramolecular H-bonding molecules are not associated

so B.pt decreases. Ex. Salicyl aldehyde i.e. O-Hydroxy Benzaldehyde has low B.pt due to intramolecular H-bonding than its isomers i.e. m or P-Hydroxy Salicyl aldehydes.

3. What are disproportionate reactions? Give an exampl e. A. Disproportionate Reaction: The reaction in which the same element undergoes oxidation as well as reduction

is called disproportionate reaction. Ex. 2 3 2

6 NaOH+3Cl 5NaCl NaClO 3H O→ + + . 2

Cl is reduced to Cl−

and is oxidised to 3

ClO− .

4. What is Deuterolysis? Give an example. A. Deuterolysis: Decomposition of a salt in presence of

2D O is called Deuterolysis.

Ex: ( )33 2AlCl 3D O Al OD 3DCl+ → +

( ) 334 3 2 4

Al C 12D O 4Al OD CD+ → +

5. Give the formula of Barytes and Dolamite. A. Barytes -

4BaSO ore of Ba; Dolomite -

3 3CaCO MgCO⋅ ore of Ca or Mg.

6. What is the kinetic energy of 5 moles of

2N gas at 27 C° in calories?

A. 3nRT 3 5 2 300

K.E. cal 4500 calories2 2

× × ×= = =

7. Name two important sinks for Carbon dioxide. A. Important sinks for

2CO are oceans, forests

8. Define C.O.D. and B.O.D.

A. C.O.D.: The amount of chemical oxygen in mg ( 22 7

Cr O / H− + ) required to oxidize organic as well as inorganic

pollutants present in 1 litre polluted water unit ppm. or mg/litre. B.O.D.: The amount of oxygen in mg used by micro organisms present in 1 litre polluted water during 5 days at 20 C° is called B.O.D. unit. ppm. or mg/litre

9. Write the structures of the following compounds .

(A) 3 – Chloro – 4 – Methyl hexane (B) 2 – Methoxy – 3, 3 – dibromo – 1 – Pentanol.

A. S.F. of 3-chloro-4-Methyl Hexane”

CH3 CH2 CH CH CH2 CH3

CH3 Cl

S.F. of 2-methoxy 3, 3-dibromo 1-pentanol”

CH3 CH2 C CH CH2

OCH3

Br

Br

OH

10. What is Functional Group Isomerism? Give an example . A. Functional Group Isomerism: The structural isomers which differ in functional groups are called functional

isomers. Ex: Acetone (

CH3 C CH3

O ) of propanal dehyde (3 2

CH CH CHO− − ).



MAY 2009

SECTION-A

1. What are the co-ordination numbers of NaCl and CsCl crystals?

A. C.N. of Na+ and Cl− in NaCl 6= ; C.N. of Cs+ and Cl− in CsCl 8= 2. Which gas diffuses faster among

2N ,

2O ,

4CH gases? Why?

A. Lighter gas diffuses fast 4

CH being lighter than 2

N , 2

O diffuses fast. 1

rM

∴ α .

3. Why

2H O has higher boiling point than HF?

A. 2

H O has more B.pt than HF due to presence of more number of H-bonds per mole 2

H O . Moreover in boiling

of HF all the H-bonds are not broken. 4. What volume of

2CO is obtained at STP by heating 10 gms of

3CaCO ?

A. 3 2

22.4 L STP100gm

CaCO CaO CO∆→ + . So 10 gm 3

CaCO liberates 10

22.4L100

× i.e. 2.24 L 2

CO .

5. What is Deuterolysis? Give an example of deuterolys is. A. Deuterolysis: Rf. Q.4 March 2010. 6. Write the names and formulae of two minerals of Bar ium. A. Two minerals of Ba (i) Bartyes

4BaSO (ii) witherite-

3BaCO

7. Write the structures of the following compounds :

a) 1, 2 – ethane diol b) 2 – amino – 3 – hydroxy p ropanoic acid

A. S.F. of 1,2-ethane diol CH CH2 2

OH OH| |

− S.F. of 2-amino-3-hydroxy propanoic acid

CH2 CH COOH

OH NH2 .

8. Write the names of the products A and B formed in t he following reaction:

Br CClAlc.KOH 2 42 5

C H Cl A B→ →

A.

( )

CH CH2 2Br CClalc.KOH 2 42 5 2 2

Br BrA(B)

C H Cl CH CH | |−

∆→ = → . A = Ethylene; B = 1,2 dibromo ethane.

9. What is the harm caused by CFC’s? A. Harmful effects of CFC; Chlorine free radical formed from CFC in stratosphere depletes ozone sphere. Which

leads to formation of holes in ozone sphere. More U.V. radiations enter into earth surface leading to destruction of life on earth surface.

10. What are COD and BOD? A. C.O.D. & B.O.D. : Ref. Q. 8 of March 2010.



MARCH 2009

SECTION – A

1. Find the volume of 3 gm of 2

H at STP.

A. Vol. of 3 gm 2

H at STP: H2

wt 3V 22.4lit 22.4 33.6lit

GMW 2= × = × =

2. Calculate the oxidation number of Oxygen in the fol lowing. (i)

2O (ii)

2OF

A. 0.N of oxygen in (i) 2

O is zero (ii) 2

OF it is +2.

3. What is the cause of hardness of water?

A. Reasons for Hardness of water: presence of 3

HCO− , Cl− , 24

SO− of 2Mg+ , 2Ca+ causes hardness of water.

4. Why the carbide of Be is called Methanide? A. Carbide of Be is called Methanide because on reaction with

2H O it liberates

4CH

( )22 2 4Be C 4H O 2Be OH CH+ → + .

5. Graphite is good conductor. Explain.

A. In Graphite carbon is 2Sp hybridized. It has layer structure. Adjacent layers are bonded weakly by π - electrons so it is soft and good conductor of electricity.

6. Write an equation for the reaction of

2SiO with Quick Lime.

A. Reaction of 2

SiO with quick lime. 2 3

SiO CaO CaSiO∆+ → (calcium silicate)

7. Explain the Nalgonda Defluoridation technique. A. Nalgonda Defluoridation Technique: ref. q. 7 of June 2010. 8. How Methyl benzene is prepared from Benzene? A. Preparation of Methyl Benzene (Toluenes) from benzene: Benzene reacts with methyl chloride in presence.

3AlCl or

3FeCl to form toluene. This reaction is called Friedel Craft alkylation.

+CH3ClFeCl3 or

AlCl3

CH3

+HCl

9. What happens when CO concentration is increased in atmosphere? A. Effect of increase in concentration of CO in atmosphere: CO reacts with Haemoglobin to form stable carboxy

Haemoglobin. Due to this supply of oxygen to brain cells decreases leading to unconsciousness finally to death.

10. Write the names of the following compounds accordin g to IUPAC rules.

a)

CH2

OH

CH2

OH b) 3 3

CH COCH

A.

CH2 CH2

OH OHEthane 1, 2-diol CH3 C CH3

O

propanone



THERMODYNAMICS

1. What is the information given by the term thermo dynamics? A. Thermodynamics gives the information of energy changes involved in a chemical reaction (or) process.

The laws of thermodynamics deal with energy changes of macroscopic systems involving a large number of molecules.

2. Define a system. Give an example. A. System: A small part of the universe chosen for thermodynamic study is called system. 3. The wall is adiabatic and adU W∆ = . What do you understand about the heat and work wi th respect to

the system? A. In adiabatic process there is no transfer of heat between system and surroundings. Work done adiabatic process is the change internal energy of the system. Work done is adabatic process 2 1adW U U U= − =∆ 4. What is the workdone in the free expansion of an ideal gas in reversible and irreversible processes ? A. In case of free expansion of an ideal gas pressure becomes zero. (into vaccum). ∴ no workdone during free expansion of an ideal gas in case to reversible as well as irreversible process. 5. State the first law of the thermodynamics. A. First Law of thermodynamics: The law of conservation of energy is taken as the first law of thermodynamics. Statements: i) “Energy can neither be created nor destroyed, although it can be transformed from one form to another”. ii) “It is impossible to construct perpetual motion machine of first kind”. iii) “The total energy of the system and surroundings in constant”. 6. What are the sign conventions of the work done o n the system and work done by the system? A. Work done on the system uses positive sign. Work done by the system uses negative sign. 7. What are the ‘ H∆ ’ sign conventions for exothermic and endothermic r eactions? A. Compounds which liberate heat in their formation reaction from the constituent elements are called exothermic

compounds. For this reactions, fH negative∆ =

Compounds which absorb heat in the formation reaction from constituent elements are called endothermic compounds. For this reactions, fH positive∆ =

8. Give the equation that gives the relationship be tween U∆ and H∆ . A. The equation that gives the relationship between U∆ and H∆ . H U nRT∆ =∆ +∆ H∆ = change in enthalpy U∆ = change in internal energy P Rn n n∆ = − , R = universal gas constant T = temperature 9. What is the relationship between pC and vC ?

A. p vC C R− =

pC = heat capacity at constant pressure

vC = heat capacity at constant volume R = universal gas constant 10. Enthalpy decrease is not the criterion for spon taneity. Why? A. Change in enthalpy “( H∆ )=negative” may be a condition but not a necessary and sufficient condition for the

spontaneous nature of a reaction. 11. Is increase of entropy the criterion for sponta neity? Why? A. Change in entropy “( S∆ )=positive” is a condition but is not necessary and sufficient condition for the

spontaneous nature of a reaction.



12. Explain the relationship between Gibbs energy c hange and equilibrium constant. A. 2.303 logkG RT∆ °=

G∆ = change in Gibbs free energy K = Equilibrium constant

13. State the third law of thermodynamics . A. Third law of thermodynamics: “The entropy of a pure and perfectly crystalline substance is zero at the absolute

zero of a temperature ( 273 C− ° )”.

lim 0 0TS → = This law imposes a limitation on the value of entropy.

0

.

TP

TC

S dTT

= ∫

14. What is Entropy? Explain with examples. A. Entropy (S): Entropy is taken as a measure of disorder of molecules (or) randomness of the system.

Greater the disorder of molecules in a system, the higher is the entropy. Entropy is a state function. It depends on the temperature, pressure of the state.

Entropy changes, revqS

T∆ = . [ revq = heat absorbed by the system isothermally and reversibly at T]

For a spontaneous process in an isolated system the entropy change is positive. ( S∆ = positive)

total system surroundingsS S S∆ =∆ +∆

Ex: heat heat

(low entropy) (moderate) (high entropy)

Solid liquid vapour→ →

15. Explain Gibbs energy. A. Gibbs energy ( G∆ ): The amount of energy available from a system which can be put to useful work at

constant temperature and pressure is called Gibb’s energy. For explaining the criteria for spontaneity of a reaction, Gibb’s introduced thermodynamic function which involved both enthalpy (H) and entropy (S) functions. This is known as free energy function (G). This is given by the equation, G H Ts= − Where ‘G’ is known as Gibbs energy (or) Gibbs function. G H T S∆ =∆ − ∆

sysG∆ = negative for spontaneous reactions ( 0G∆ < )

sysG∆ = positive for non-spontaneous reactions ( 0G∆ > )

sysG∆ = zero equilibrium reactions ( 0G∆ = )

CHEMICAL EQUILIBRIUM

1. State law of chemical equilibrium. A. The ratio of product of molar concentrations of the products to the product of molar concentrations of the

reactants has a constrant value. This is known as the equilibrium law (or) law of chemical equilibrium. 2. Can equilibrium be achieved between water and it s vapours in an open vessel. Explain. A. Equilibrium does not achieved between water and its vapour in an open vessel.

But the equilibrium achieved between water and its vapour in a closed vessel.

( ) ( )2 2l gH O H O⇌

3. Why the concentrations of pure liquids and pure solids are ignored from equilibrium constant

expressions? A. The concentrations of pure solids and pure liquids are ignored from equilibrium constant expressions because

the concentrations of pure solid and pure liquids are taken as unity. 4. Define equilibrium constant. A. The ratio of product of molar concentrations of products to the product of molar concentrations of reactants is

called equilibrium constant ( )cK .



5. Write the relation between pK and cK .

A. ( ) nP CK K RT ∆=

n∆ =No. of gaseous products – No. of gaseous reactants R=universal gas constant

6. Under what conditions for a reaction PK and SK are numerically equal?

A. If n O∆ = i.e. No. of gaseous products = No. of gaseous reactants then ( ) nP CK K RT ∆=

( )OP CK K RT=

P CK K=

7. Give two chemical equilibrium reactions for whic h P CK K w<

A. 1) ( ) ( ) ( )2 2 33 2g g gN H NH+ ⇌

( )2 1 3 2P Rn n n∆ = − = − + =−

( )2n ve∆ =− −

P CK K∴ <

2) ( ) ( ) ( )2 2 32 2g g gSO O SO+ ⇌

( )2 1 2 1P Rn n n∆ = − = − + =−

( )1n ve∆ =− −

P CK K∴ <

8. What are the factors which influence the chemica l equilibrium? A. The factors influencing chemical equilibrium are

1) concentration of reactants and the products 2) temperature of reaction 3) pressure of reaction 4) inert gas addition etc.

9. The equilibrium constants of a reaction at 27 C° and at 127 C° are 31.6 10−× and 27.6 10−× respectively. Is the reaction exothermic or endothe rmic.

A. Given equilibrium constants

At 327 1.6 10C −° − ×

At 2127 7.6 10C −° − × From the above values as the temperature raised equilibrium constant value increased. Here H ve∆ =+ ∴ the reaction is endothermic.

10. What is a Bronsted base? Give one example. A. The substance which accepts a proton from the other substance is called Bronsted base. e.g.: 3 2,NH H O etc. 11. What is Lewis acid? Give one example. A. A substance which can accept an electron pair to from a coordinate covalent bond with donor is called Lewis

acid. e.g. 3 2, ,H BF SnCl+ etc.

12. What is meant by ionic product of water?

A. At a given temp. the product of the concentrations of H+ and OH− ions in water is called ionic product.

Ionic product wK H OH+ − =

At 25 C° 14 2 21.008 10wK mole lit−= ×

13. What is the value of WK ? What are its units?

A. At 25 C° ionic product of water 14 2 21.008 10wK mole lit−= ×

Units : 2 2mole lit



14. 2 2 3⇌H O H O H O OH+ −

+ +

The ionic product of water is 141 10−× at 25 C° and 143.0 10−× at 40 C° . Is the above process endothermic or exothermic?

A. Given reaction

2 2 3H O H O H O OH+ −+ +⇌

wK at 25 C° - 14 2 21 10 mole lit−×

wK at 40 C° - 14 2 23 10 mole lit−×

The above reaction is endothermic reaction because wK value increases with increase of temperature.

15. All Lewis acids are not Bronsted acids. Why? A. Lewis Acid means electron pair acceptor and bronsted acid means proton donor.

According to Lewis concept many acids do not have proton. So all Lewis acids are not Bronsted bases.

16. Give two examples of salts whose aqueous soluti ons are basic. A. Sodium acetate ( )3CH COONa , sodium carbonate ( )2 3Na CO salts aqueous solutions are basic in nature

due to anionic hydrolysis. 17. Ice melts slowly at high altitudes. Explain. Wh y? A. Ice melts slowly at high altitudes.

Reason: Ice and water are equilibrium only at a particular temperature and pressure conditions. At high attitude temperature and pressure conditions are changed.

18. Why is it useful to compare Q with K? A. Q and K are compared to predict the direction of reaction

a) Q = K indicates that the reaction mixture is already at equilibrium. b) Q K< indicates that the reaction proceeds in the direction.

c) Q K> indicates that the reaction proceeds in the direction of reactants (Reverse reaction).

19. Explain the Arrhenius concept of acids and base s. A. According to Arrhenius

Acid: Acids are the substances that dissociates in water to gave H+ ions. e.g.: 2 4,HCl H SO etc…

( ) ( ) ( )aq aq aqHx H x+→ +

Bases: Bases are the substances that produce hydrorylions (OH− ) ion dissociation in water. e.g. : NaOH, KOH

( ) ( ) ( )aq aq aqMOH M OH+ −→ +

20. Show by suitable equations that each of the fol lowing species can act as a Bronsted acid.

A. a) 3 2H O H O H+ +→ +

Proton donar hence a bronsted acid

b) HCl H Cl+ −→ + Proton donar hence a bronsted acid c) 3NH is bronsted base it’s not an acid

(Sometimes 3 2NH NH H− +→ + as acid)

d) 4 4HSO H SO− + −→ +

Proton donar hence bronsted acid

Note: All very short questions from TEXT BOOK. All In text solved problems.



SHORT ANSWER TYPE QUESTIONS

PAGE NO. QUESTION NO. TOPIC NAME

422, 423, 424 26, 29, 30, 31, 34, 40, 42, 43, 44, 49,

50, 51, 52, 53, 54, 55, 57, 60, 63, 64, 65 ORGANIC CHEMISTRY

139, 140, 141 48, 49, 50, 51, 52, 53, 54, 55, 65, 69

(In text Solved Problems) GASEOUS STATE

185 TO 190

16, 17, 18, 19, 23, 24, 25, 29, 30, 31,

33, 56, 61, 62, 70, 71, 72, 73, 74, 75,

76, 77, 78, 81, 82

STOICHIOMETRY

221 TO 225 39, 40, 44, 45, 47, 52, 53, 54, 62, 78,

79, 81, 83, 88, 90, 93, 95, 96, 97, 98 THERMODYNAMICS

268 TO 278

39, 40, 43, 53, 58, 70, 74, 75, 78, 79,

87, 89, 91, 97, 98, 99 (In text solved

problems)

CHEMICAL EQUILIBRIUM,

ACIDS-BASES

292, 293 15, 17, 26, 29, 31, 32, 33 HYDROGEN AND ITS

COMPOUNDS

308, 309 33, 34, 38, 39, 41 S-BLOCK ELEMENTS

319, 320, 321 9, 16, 25, 26, 28, 37, 38, 39 P-BLOCK ELEMENTS

LONG ANSWER TYPE QUESTIONS

PAGE NO. QUESTION NO. TOPIC NAME

42 & 43 53, 54, 55, 61, 67 ATOMIC STRUCTURE

73 & 74 83, 85, 87, 88, 90, 91, 92, 93, 94 PERIODIC TABLE

110 40, 41, 43, 44, 45, 46, 47, 48 CHEMICAL BOND

422 28, 32, 33, 36, 37, 38, 39, 45, 47, 48 ORGANIC CHEMISTRY

Wwish you all the bestX

Documents

FIRST YEAR - IPE CHEMISTRY - FIITJEE Hyderabad YEAR - IPE CHEMISTRY `KUKATPALLY CENTRE Total No. of Questions - 21 Reg. Total No. of Printed Pages - 2 No. Paper - I CHEMISTRY IPE BOARD