Final Exam Review Units 5-8. Warm Up Go to the blog Click on the Day 2 WARM UP Questions While you are waiting to begin, review your stations from yesterday

Final Exam ReviewUnits 5-8

Warm Up

• Go to the blog• Click on the Day 2 WARM UP Questions• While you are waiting to begin, review your

stations from yesterday.

Station 1 (Moles Unit 5)

• Complete the below Mole Map:

Mole

Volume

MassParticles


• Complete the below Mole Map:

Mole

Volume

MassParticles


Convert 4.5 g CO2 to molecules.

a) 6.2x1020 moleculesb) 6.2x1022 moleculesc) 1.2x10-25 moleculesd) 1.2x1025 molecules

Calculate the mass of 4.3L of oxygen gas.

a) 3.1 gramsb) 6.1 gramsc) 31 g ramsd) 61 gramse) 138 grams


Convert 4.5 g CO2 to molecules.

a) 6.2x1020 moleculesb) 6.2x1022 moleculesc) 1.2x10-25 moleculesd) 1.2x1025 molecules

Calculate the mass of 4.3L of oxygen gas.

a) 3.1 gramsb) 6.1 gramsc) 31 g ramsd) 61 gramse) 138 grams


1. Define molecular formula.2. Define empirical formula.3. How do you find empirical formula given the

percent composition? (remember the rhyme)4. Once you have empirical formula how do you

find molecular formula? What other information do you need?


1. The actual formula of the compound2. The formula of the compound with reduced

subscripts. Its based on the percent composition.3. % to grams; gram to mole; divide by smallest;

multiply till whole4. Find the molar mass of the empirical formula and

compare it to the given molar mass of the compound (this is the additional information you need). If different, multiply subscripts by their quotient.


A compound consisting of C, H, and O is found to contain 40.00% C and 6.71% H. Determine the empirical formula of the compound.

a) CH2O

b) CHOc) C2H4O2

d) C6H12O6

e) CH2

The molecular mass of the compound to the left is calculated to be 180.0 g/mol. Determine the molecular formula of the compound.

a) CH2O

b) C3H6O3

c) C2H4O2

d) C6H12O6

e) C18H36O18


A compound consisting of C, H, and O is found to contain 40.00% C and 6.71% H. Determine the empirical formula of the compound.

a) CH2O

b) CHOc) C2H4O2

d) C6H12O6

e) CH2

The molecular mass of the compound to the left is calculated to be 180.0 g/mol. Determine the molecular formula of the compound.

a) CH2O

b) C3H6O3

c) C2H4O2

d) C6H12O6

e) C18H36O18

Station 3 (Stoichiometry Unit 6)

1. What conversion factor do you use to convert between moles of different elements within a given reaction?

2. What do you need to make sure is done before you use the above factor?

3. How do you determine the limiting reactant?

Station 3 (Stoichiometry Unit 6)

1. Mole ratio2. Balanced equation3. Solve the stoichiometry problem to find the

mass of the product for each given reactant. The number that gives you the smallest answer is the limiting reactant.

Station 3 (Stoichiometry Unit 6)P4 + 5O2 P4O10

Determine the mass of tetraphosphorus decoxide formed if 25.0 g of phosphorus (P4) and 50.0 g of oxygen gas are combined.a) 57.3 grams of P4O10

b) 88.7 grams of P4O10

c) 146 grams of P4O10

d) 25.0 grams of P4O10

e) 50.0 grams of P4O10

Which reactant is limiting in the example to the left?

a) 25.0 g of P4

b) 50.0g of O2

c) 57.3 g of P4O10


Station 3 (Stoichiometry Unit 6)P4 + 5O2 P4O10

Determine the mass of tetraphosphorus decoxide formed if 25.0 g of phosphorus (P4) and 50.0 g of oxygen gas are combined.a) 57.3 grams of P4O10

b) 88.7 grams of P4O10

c) 146 grams of P4O10


e) 50.0 grams of P4O10

Which reactant is limiting in the example to the left?

a) 25.0 g of P4

b) 50.0g of O2

c) 57.3 g of P4O10


Station 4 (Heat Unit 7)

1. What is the equation that relates heat to change in temperature?

2. Define endothermic3. Define exothermic


1. Q=mcΔT2. Endothermic requires heat to be added to

proceed3. Exothermic releases heat


• Which of the following is an endothermic phase change?

a) Sublimationb) Freezingc) Condensationd) None of these

• Which of the following is an exothermic phase change?

a) Evaporationb) Meltingc) Depositiond) None of these


• Which of the following is an endothermic phase change?

a) Sublimationb) Freezingc) Condensationd) None of these

• Which of the following is an exothermic phase change?

a) Evaporationb) Meltingc) Depositiond) None of these


How much heat does a 3.0 grams of water absorb as its temperature increases from 0C to 5.0C?

a) 88.54 Jb) 3.59 Jc) 20.92 Jd) 62.76 J

A 25 g sample of water is absorbs 942 J as it is heated. If the initial temperature of the water was 23.5oC, what is the final temp?a. 9.01 oCb. 32.51 oCc. 157.7 oCd. 134.15 oC

cice=2.1 J/goC, cwater=4.184 J/goC, csteam=1.7 J/goC


How much heat does a 3.0 grams of water absorb as its temperature increases from 0C to 5.0C?

a) 88.54 Jb) 3.59 Jc) 20.92 Jd) 62.76 J

A 25 g sample of water is absorbs 942 J as it is heated. If the initial temperature of the ethanol was 23.5oC, what is the final temp?a. 9.01 oCb. 32.51 oCc. 157.7 oCd. 134.15 oC

cice=2.1 J/goC, cwater=4.184 J/goC, csteam=1.7 J/goC

Station 5 (Solutions Unit 8)

1. What factors affect the rate of solvation (ie. the rate at which a solvent dissolves)?

2. Define molarity. What are its units?3. Define molality. What are its units?


1. Agitation (stirring), increasing temperature (heating), increasing surface area (crushing), all increase the rate of solvation.

2. . It has units of mol/L or M.3. . It has units of mol/kg or m.


What is the volume of solution if the molarity is 0.45M and 0.15 moles of solute are dissolved?

a) 0.33 L of solutionb) 0.33 mL of solutionc) 3.00 L of solutiond) 3.00 mL of solutione) None of these

Calculate the molarity of a solution if 1500 g of H2SO4 is dissolve in 5.0L of water.

a. 300 Mb. 0.3 Mc. 3.06 Md. 0.003 M


What is the volume of solution if the molarity is 0.45M and 0.15 moles of solute are dissolved?

a) 0.33 L of solutionb) 0.33 mL of solutionc) 3.00 L of solutiond) 3.00 mL of solutione) None of these

Calculate the molarity of a solution if 1500 g of H2SO4 is dissolve in 5.0L of water.

a. 300 Mb. 0.3 Mc. 3.06 Md. 0.003 M


What is the mass of NaOH needed to prepare a 3500mL solution of 0.66 M NaOH?

a. 2310 gb. 92.4 gc. 0.0924 gd. 2.31 g

What is the volume of a 0.56M solution containing and 80 grams of NaOH?

a. 3.57 Lb. 35.7mLc. 142.8 Ld. 14.3 L


What is the mass of NaOH needed to prepare a 3500mL solution of 0.66 M NaOH?

a. 2310 gb. 92.4 gc. 0.0924 gd. 2.31 g

What is the volume of a 0.56M solution containing and 80 grams of NaOH?

a. 3.57 Lb. 35.7mLc. 142.8 Ld. 14.3 L

Station 6 (Acid/Base Unit 8)

1. What is the Arrhenius definition of an acid?2. What is the Arrhenius definition of a base?3. What is the Bronstead-Lowry definition of an

acid?4. What is the Bronstead-Lowry definition of a

base?


1. Produces H+ ion2. Produces OH- ion3. H+ ion donor4. H+ ion acceptor


According to the Arrhenius theory a substance that releases a hydrogen ion is classified as a(n)

a) Acidb) Basec) Conjugate Acidd) Conjugate Base

Consider the reaction:NH3(aq) + H2O(l) NH4

+(aq) + OH-(aq)

What species is the conjugate acid?

a) NH3

b) H2O

c) NH4+

d) OH-


According to the Arrhenius theory a substance that releases a hydrogen ion is classified as a(n)

a) Acidb) Basec) Conjugate Acidd) Conjugate Base

Consider the reaction:NH3(aq) + H2O(l) NH4

+(aq) + OH-(aq)

What species is the conjugate acid?

a) NH3

b) H2O

c) NH4+

d) OH-


• What is the pH range for an acid? Base?• Complete the following map:

[H+] pH

[OH-] pOH


• What is the pH range for an acid? Base?• Complete the following map:

[H+] pH

[OH-] pOH


If the [H+] is equal to 9.2 x 10 -4 M, it’s a(n) _________

a) Acidb) Basec) Neutral solution

Calculate the [OH-] for a solution that has [H+] is equal to 2.0 x 10 -8 M

a. 5.0 x 10-1 Mb. 5.0 x 10-7 Mc. 1.0 x10-7 Md. 2.0 x 10-7 M


If the [H+] is equal to 9.2 x 10 -4 M, it’s a(n) _________

a) Acidb) Basec) Neutral solution

Calculate the [OH-] for a solution that has [H+] is equal to 2.0 x 10 -8 M

a. 5.0 x 10-1 Mb. 5.0 x 10-7 Mc. 1.0 x10-7 Md. 2.0 x 10-7 M

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Final Exam Review Units 5-8. Warm Up Go to the blog Click on the Day 2 WARM UP Questions While you are waiting to begin, review your stations from yesterday