Question 1

What volume of a 0.540 mol L-1 NaOH solution contains 11.5 g of NaOH?

Accepted Answer

A) 0.155 L 
B) 0.532 L 
C) 1.88 L 
D) 6.44 L 
A) 0.155 L 
B) 0.532 L 
C) 1.88 L 
D) 6.44 L B

Question 2

How many millilitres of a stock solution of 11.1 mol L-1 HNO3 would be needed to prepare 0.500 L of 0.500 mol L-1 HNO3?

Accepted Answer

A) 0.0444 
B) 22.5 
C) 2.78 
D) 44.4 
E) 0.0225 
A) 0.0444 
B) 22.5 
C) 2.78 
D) 44.4 
E) 0.0225 B

Question 3

How many grams of AgNO3 are needed to make 250. mL of a solution that is 0.135 mol L-1?

Accepted Answer

A) 0.0917 g 
B) 0.174 g 
C) 5.73 g 
D) 91.7 g 
A) 0.0917 g 
B) 0.174 g 
C) 5.73 g 
D) 91.7 g C

Question 4

What are the required coefficients to properly balance the following chemical reaction? 
N2H4(l)→ NH3(g)+ N2(g)

Accepted Answer

A) 3, 4, 1 
B) 2, 3, 2 
C) 3, 4, 4 
D) 1, 4, 3 
E) 2, 2, 1 
A) 3, 4, 1 
B) 2, 3, 2 
C) 3, 4, 4 
D) 1, 4, 3 
E) 2, 2, 1

Question 5

Which of the following is considered a strong electrolyte?

Accepted Answer

A) NH4NO3 
B) C12H22O11 
C) PbCl2 
D) HC2H3O2 
E) CH3OH 
A) NH4NO3 
B) C12H22O11 
C) PbCl2 
D) HC2H3O2 
E) CH3OH

Question 6

In an acid-base neutralization reaction, 38.74 mL of 0.500 mol L-1 potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution?

Accepted Answer

A) 0.194 mol L-1 
B) 0.387 mol L-1 
C) 0.775 mol L-1 
D) 1.29 mol L-1 
A) 0.194 mol L-1 
B) 0.387 mol L-1 
C) 0.775 mol L-1 
D) 1.29 mol L-1

Question 7

What are the required coefficients to properly balance the following chemical reaction? 
C6H12O6(s)+ O2(g)→ CO2(g)+ H2O(l)

Accepted Answer

A) 1, 3, 3, 3 
B) 2, 6, 6, 3 
C) 1, 6, 6, 6 
D) 1, 1, 3, 3 
E) 2, 2, 6, 3 
A) 1, 3, 3, 3 
B) 2, 6, 6, 3 
C) 1, 6, 6, 6 
D) 1, 1, 3, 3 
E) 2, 2, 6, 3

Question 8

A student dissolved 4.00 g of Co(NO3)2 in enough water to make 100. mL of stock solution. He took 4.00 mL of the stock solution and then diluted it with water to give 275. mL of a final solution. How many grams of NO3- ion are there in the final solution?

Accepted Answer

A) 0.0197 g 
B) 0.0394 g 
C) 0.0542 g 
D) 0.108 g 
A) 0.0197 g 
B) 0.0394 g 
C) 0.0542 g 
D) 0.108 g

Question 9

Identify the balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate.

Accepted Answer

A) Al(C2H3O2)2(aq)+ (NH4)2PO4(aq)→ AlPO4(s)+ 2NH4C2H3O2(aq) 
B) Al(C2H3O2)2(aq)+ (NH3)2PO4(aq)→ AlPO4(s)+ 2NH3C2H3O2(aq) 
C) Al(CO3)2(aq)+ (NH3)2PO4(aq)→ AlPO4(s)+ 2NH3CO3(aq) 
D) Al(C2H3O2)3(aq)+ (NH4)3PO4(aq)→ AlPO4(s)+ 3NH4C2H3O2(aq) 
E) Al(CO2)3(aq)+ (NH4)3PO3(aq)→ AlPO3(s)+ 3NH4CO2(aq) 
A) Al(C2H3O2)2(aq)+ (NH4)2PO4(aq)→ AlPO4(s)+ 2NH4C2H3O2(aq) 
B) Al(C2H3O2)2(aq)+ (NH3)2PO4(aq)→ AlPO4(s)+ 2NH3C2H3O2(aq) 
C) Al(CO3)2(aq)+ (NH3)2PO4(aq)→ AlPO4(s)+ 2NH3CO3(aq) 
D) Al(C2H3O2)3(aq)+ (NH4)3PO4(aq)→ AlPO4(s)+ 3NH4C2H3O2(aq) 
E) Al(CO2)3(aq)+ (NH4)3PO3(aq)→ AlPO3(s)+ 3NH4CO2(aq)

Question 10

How many millilitres of 0.132 mol L-1 HClO4 solution are needed to neutralize 50.00 mL of 0.0789 mol L-1 NaOH?

Accepted Answer

A) 0.521 
B) 0.0120 
C) 83.7 
D) 0.0335 
E) 29.9 
A) 0.521 
B) 0.0120 
C) 83.7 
D) 0.0335 
E) 29.9

Question 11

What reagent could be used to separate Br- from CH3CO2- when added to an aqueous solution containing both?

Accepted Answer

A) AgNO3(aq) 
B) Ba(OH)2(aq) 
C) CuSO4(aq) 
D) NaI(aq) 
A) AgNO3(aq) 
B) Ba(OH)2(aq) 
C) CuSO4(aq) 
D) NaI(aq)

Question 12

What element is undergoing oxidation (if any)in the following reaction? CH4(g)+ 2O2(g)→ CO2(g)+ 2H2O(g)

Accepted Answer

A) O 
B) H 
C) C 
D) both C and H 
E) None of the elements is undergoing oxidation. 
A) O 
B) H 
C) C 
D) both C and H 
E) None of the elements is undergoing oxidation.

Question 13

Determine the limiting reactant (LR)and the mass (in g)of nitrogen that can be formed from 50.0 g N2O4 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g mol-1, N2H4 = 32.05 g mol-1. N2O4(l)+ 2N2H4(l)→ 3N2(g)+ 4H2O(g)

Accepted Answer

A) LR = N2H4, 59.0 g N2 formed 
B) LR = N2O4, 105 g N2 formed 
C) LR = N2O4, 45.7 g N2 formed 
D) LR = N2H4, 13.3 g N2 formed 
E) No LR, 45.0 g N2 formed 
A) LR = N2H4, 59.0 g N2 formed 
B) LR = N2O4, 105 g N2 formed 
C) LR = N2O4, 45.7 g N2 formed 
D) LR = N2H4, 13.3 g N2 formed 
E) No LR, 45.0 g N2 formed

Question 14

Which of the compounds H2C2O4, Ca(OH)2, KOH, and HI behave as bases when they are dissolved in water?

Accepted Answer

A) Ca(OH)2 and KOH 
B) H2C2O4 and HI 
C) only HI 
D) only KOH 
A) Ca(OH)2 and KOH 
B) H2C2O4 and HI 
C) only HI 
D) only KOH

Question 15

How many grams of CaCl2 are formed when 15.00 mL of 0.00237 mol L-1 Ca(OH)2 reacts with excess Cl2 gas? 2Ca(OH)2(aq)+ 2Cl2(g)→ Ca(OCl)2(aq)+ CaCl2(s)+ 2H2O(l)

Accepted Answer

A) 0.00197 g 
B) 0.00394 g 
C) 0.00789 g 
D) 0.0507 g 
A) 0.00197 g 
B) 0.00394 g 
C) 0.00789 g 
D) 0.0507 g

Question 16

Determine the oxidation state of C in CO3-2.

Accepted Answer

A) +4 
B) +2 
C) -2 
D) -4 
E) +6 
A) +4 
B) +2 
C) -2 
D) -4 
E) +6

Question 17

Identify the percent yield when 28.16 g of CO2 are formed from the reaction of 8.000 moles of C8H18 with 4.000 moles of O2. 2C8H18 + 25O2 → 16CO2 + 18H2O

Accepted Answer

A) 20.00% 
B) 25.00% 
C) 50.00% 
D) 12.50% 
A) 20.00% 
B) 25.00% 
C) 50.00% 
D) 12.50%

Question 18

Balance the following equation:
_____ C9H20 + _____ O2  → _____ H2O + _____ CO2

Accepted Answer

C₉H₂₀ + 14O₂ →

Question 19

Explain the difference between a strong and weak electrolyte. Give an example of each.

Accepted Answer

A strong electrolyte is either an ionic

Question 20

How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g mol-1. 4KNO3(s)→ 2K2O(s)+ 2N2(g)+ 5O2(g)

Accepted Answer

A) 0.290 mol N2 
B) 0.580 mol N2 
C) 18.5 mol N2 
D) 0.724 mol N2 
E) 1.73 mol N2 
A) 0.290 mol N2 
B) 0.580 mol N2 
C) 18.5 mol N2 
D) 0.724 mol N2 
E) 1.73 mol N2

Exam 4: Chemical Reactions and Stoichiometry

What volume of a 0.540 mol L-1 NaOH solution contains 11.5 g of NaOH?

How many millilitres of a stock solution of 11.1 mol L-1 HNO3 would be needed to prepare 0.500 L of 0.500 mol L-1 HNO3?

How many grams of AgNO3 are needed to make 250. mL of a solution that is 0.135 mol L-1?

What are the required coefficients to properly balance the following chemical reaction? N2H4(l)→ NH3(g)+ N2(g)

Which of the following is considered a strong electrolyte?

In an acid-base neutralization reaction, 38.74 mL of 0.500 mol L-1 potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution?

What are the required coefficients to properly balance the following chemical reaction? C6H12O6(s)+ O2(g)→ CO2(g)+ H2O(l)

A student dissolved 4.00 g of Co(NO3)2 in enough water to make 100. mL of stock solution. He took 4.00 mL of the stock solution and then diluted it with water to give 275. mL of a final solution. How many grams of NO3- ion are there in the final solution?

Identify the balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate.

How many millilitres of 0.132 mol L-1 HClO4 solution are needed to neutralize 50.00 mL of 0.0789 mol L-1 NaOH?

What reagent could be used to separate Br- from CH3CO2- when added to an aqueous solution containing both?

What element is undergoing oxidation (if any)in the following reaction? CH4(g)+ 2O2(g)→ CO2(g)+ 2H2O(g)

Determine the limiting reactant (LR)and the mass (in g)of nitrogen that can be formed from 50.0 g N2O4 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g mol-1, N2H4 = 32.05 g mol-1. N2O4(l)+ 2N2H4(l)→ 3N2(g)+ 4H2O(g)

Which of the compounds H2C2O4, Ca(OH)2, KOH, and HI behave as bases when they are dissolved in water?

How many grams of CaCl2 are formed when 15.00 mL of 0.00237 mol L-1 Ca(OH)2 reacts with excess Cl2 gas? 2Ca(OH)2(aq)+ 2Cl2(g)→ Ca(OCl)2(aq)+ CaCl2(s)+ 2H2O(l)

Determine the oxidation state of C in CO3-2.

Identify the percent yield when 28.16 g of CO2 are formed from the reaction of 8.000 moles of C8H18 with 4.000 moles of O2. 2C8H18 + 25O2 → 16CO2 + 18H2O

Balance the following equation: _____ C9H20 + _____ O2 → _____ H2O + _____ CO2

Explain the difference between a strong and weak electrolyte. Give an example of each.

How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g mol-1. 4KNO3(s)→ 2K2O(s)+ 2N2(g)+ 5O2(g)

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Filters

What volume of a 0.540 mol L^-1 NaOH solution contains 11.5 g of NaOH?

How many millilitres of a stock solution of 11.1 mol L^-1 HNO₃ would be needed to prepare 0.500 L of 0.500 mol L^-1 HNO₃?

How many grams of AgNO₃ are needed to make 250. mL of a solution that is 0.135 mol L^-1?

What are the required coefficients to properly balance the following chemical reaction? N₂H₄(l)→ NH₃(g)+ N₂(g)

In an acid-base neutralization reaction, 38.74 mL of 0.500 mol L^-1 potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H₂SO₄ solution?

What are the required coefficients to properly balance the following chemical reaction? C₆H₁₂O₆(s)+ O₂(g)→ CO₂(g)+ H₂O(l)

A student dissolved 4.00 g of Co(NO₃)₂ in enough water to make 100. mL of stock solution. He took 4.00 mL of the stock solution and then diluted it with water to give 275. mL of a final solution. How many grams of NO₃^- ion are there in the final solution?

How many millilitres of 0.132 mol L^-1 HClO₄ solution are needed to neutralize 50.00 mL of 0.0789 mol L^-1 NaOH?

What reagent could be used to separate Br^- from CH₃CO₂^-when added to an aqueous solution containing both?

What element is undergoing oxidation (if any)in the following reaction? CH₄(g)+ 2O₂(g)→ CO₂(g)+ 2H₂O(g)

Determine the limiting reactant (LR)and the mass (in g)of nitrogen that can be formed from 50.0 g N₂O₄ and 45.0 g N₂H₄. Some possibly useful molar masses are as follows: N₂O₄ = 92.02 g mol^-1, N₂H₄ = 32.05 g mol^-1. N₂O₄(l)+ 2N₂H₄(l)→ 3N₂(g)+ 4H₂O(g)

Which of the compounds H₂C₂O₄, Ca(OH)₂, KOH, and HI behave as bases when they are dissolved in water?

How many grams of CaCl₂ are formed when 15.00 mL of 0.00237 mol L^-1 Ca(OH)₂ reacts with excess Cl₂ gas? 2Ca(OH)₂(aq)+ 2Cl₂(g)→ Ca(OCl)₂(aq)+ CaCl₂(s)+ 2H₂O(l)

Determine the oxidation state of C in CO₃^-2.

Identify the percent yield when 28.16 g of CO₂ are formed from the reaction of 8.000 moles of C₈H₁₈ with 4.000 moles of O₂. 2C₈H₁₈ + 25O₂→ 16CO₂ + 18H₂O

Balance the following equation: ___ C₉H₂₀ + _ O₂ → _ H₂O + ___ CO₂

How many moles of nitrogen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s)→ 2K₂O(s)+ 2N₂(g)+ 5O₂(g)