Question 1

Identify the polyprotic acid.

Accepted Answer

A)  H2SO4 
B)  HCl 
C)  NaCl 
D)  NaOH 
E)  Li(OH)2 
A)  H2SO4 
B)  HCl 
C)  NaCl 
D)  NaOH 
E)  Li(OH)2

Question 2

What causes a precipitation reaction to occur between two soluble compounds?

Accepted Answer

A precipitate, or insoluble co

Question 3

How many moles of oxygen 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 O2 
B)  0.580 mol O2 
C)  18.5 mol O2 
D)  0.724 mol O2 
E)  1.73 mol O2 
A)  0.290 mol O2 
B)  0.580 mol O2 
C)  18.5 mol O2 
D)  0.724 mol O2 
E)  1.73 mol O2

Question 4

What are the required coefficients to properly balance the following chemical reaction? 
CH4(g) + H2O(g) → CO(g) + H2(g)

Accepted Answer

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

Question 5

Choose the reaction that represents the combustion of C6H12O2.

Accepted Answer

A)  C6H12O2(l) + 8O2(g) → 6CO2(g) + 6H2O(g) 
B)  Mg(s) + C6H12O2(l) → MgC6H12O2(aq) 
C)  6C(s) + 6H2(g) + O2(g) → C6H12O2(l) 
D)  C6H12O2(l) → 6C(s) + 6H2(g) + O2(g) 
E)  None of the above represents the combustion of C6H12O2. 
A)  C6H12O2(l) + 8O2(g) → 6CO2(g) + 6H2O(g) 
B)  Mg(s) + C6H12O2(l) → MgC6H12O2(aq) 
C)  6C(s) + 6H2(g) + O2(g) → C6H12O2(l) 
D)  C6H12O2(l) → 6C(s) + 6H2(g) + O2(g) 
E)  None of the above represents the combustion of C6H12O2.

Question 6

Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum. 
Al(s) + I2(s) → Al2I6(s)

Accepted Answer

A)  0.741 mol 
B)  1.67 mol 
C)  2.22 mol 
D)  3.33 mol 
A)  0.741 mol 
B)  1.67 mol 
C)  2.22 mol 
D)  3.33 mol

Question 7

Identify the oxidation state of H in HCl(aq). 
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

Accepted Answer

A)  +1 
B)  +2 
C)  0 
D)  -1 
E)  -2 
A)  +1 
B)  +2 
C)  0 
D)  -1 
E)  -2

Question 8

When 280. mL of 1.50 × 10-4 mol L-1 hydrochloric acid is added to 135 mL of 1.75 × 10-4 mol L-1 Mg(OH)2, the resulting solution will be ________.

Accepted Answer

A)  acidic 
B)  basic 
C)  neutral 
D)  It is impossible to tell from the information given. 
A)  acidic 
B)  basic 
C)  neutral 
D)  It is impossible to tell from the information given.

Question 9

What is the concentration (M) of sodium ions in 4.57 L of a 1.25 mol L-1 Na3P solution?

Accepted Answer

Question 10

Determine the oxidation state of Sn in Sn(SO4)2.

Accepted Answer

A)  +2 
B)  +4 
C)  +6 
D)  0 
E)  -2 
A)  +2 
B)  +4 
C)  +6 
D)  0 
E)  -2

Question 11

Which of the following compounds is soluble in water?

Accepted Answer

A)  CaCl2 
B)  MgCO3 
C)  PbCl2 
D)  BaSO4 
E)  None of these compounds is soluble in water. 
A)  CaCl2 
B)  MgCO3 
C)  PbCl2 
D)  BaSO4 
E)  None of these compounds is soluble in water.

Question 12

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

Accepted Answer

A)  1.50 mol L-1 
B)  1.18 mol L-1 
C)  0.130 mol L-1 
D)  0.768 mol L-1 
E)  2.30 mol L-1 
A)  1.50 mol L-1 
B)  1.18 mol L-1 
C)  0.130 mol L-1 
D)  0.768 mol L-1 
E)  2.30 mol L-1

Question 13

How many millilitres of a stock solution of 13.1 mol L-1   would be needed to prepare 0.500 L of 0.500 mol L-1   ?

Accepted Answer

A)  0.0191 mL 
B)  52.4 mL 
C)  0.0524 mL 
D)  3.28 mL 
E)  19.1 mL 
A)  0.0191 mL 
B)  52.4 mL 
C)  0.0524 mL 
D)  3.28 mL 
E)  19.1 mL

Question 14

If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350. mL of solution?

Accepted Answer

A)  0.0 101 mol L-1 
B)  0. 0404 mol L-1 
C)  0. 162 mol L-1 
D)  0. 323 mol L-1 
A)  0.0 101 mol L-1 
B)  0. 0404 mol L-1 
C)  0. 162 mol L-1 
D)  0. 323 mol L-1

Question 15

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 16

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) +   (g) →   N(s)
In a particular experiment, 5.50 g samples of each reagent are reacted. What is the theoretical yield of lithium nitride?

Accepted Answer

A)  4.60 g 
B)  13.7 g 
C)  27.6 g 
D)  3.42 g 
E)  9.20 g 
A)  4.60 g 
B)  13.7 g 
C)  27.6 g 
D)  3.42 g 
E)  9.20 g

Question 17

Which of the following statements is TRUE?

Accepted Answer

A)  A reduction process corresponds to an increase in oxidation state as a result of loss of electrons. 
B)  An oxidation process involves the loss of electrons resulting in an increase in oxidation state. 
C)  An oxidation process corresponds to a decrease in oxidation state as a result of a gain of electrons. 
D)  During a reduction process electrons are lost, while during an oxidation they are gained. 
E)  During a reduction process an oxidation state increases, while in an oxidation process an oxidation state decreases. 
A)  A reduction process corresponds to an increase in oxidation state as a result of loss of electrons. 
B)  An oxidation process involves the loss of electrons resulting in an increase in oxidation state. 
C)  An oxidation process corresponds to a decrease in oxidation state as a result of a gain of electrons. 
D)  During a reduction process electrons are lost, while during an oxidation they are gained. 
E)  During a reduction process an oxidation state increases, while in an oxidation process an oxidation state decreases.

Question 18

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

Accepted Answer

C₉H₂₀ + 14O₂→

Question 19

According to the following reaction, what mass of PbCl2 can form from 235 mL of a 0.110 mol L-1 KCl solution? Assume that there is excess Pb(NO3)2. 2KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2KNO3(aq)

Accepted Answer

A)  7.19 g 
B)  3.59 g 
C)  1.80 g 
D)  5.94 g 
E)  1.30 g 
A)  7.19 g 
B)  3.59 g 
C)  1.80 g 
D)  5.94 g 
E)  1.30 g

Question 20

What are the required coefficients to properly balance the following chemical reaction? 
PbS(s) + HBr(aq) → PbBr2(s) + H2S(g)

Accepted Answer

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

Exam 4: Chemical Reactions and Stoichiometry

Identify the polyprotic acid.

What causes a precipitation reaction to occur between two soluble compounds?

How many moles of oxygen 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)

What are the required coefficients to properly balance the following chemical reaction? CH4(g) + H2O(g) → CO(g) + H2(g)

Choose the reaction that represents the combustion of C6H12O2.

Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum. Al(s) + I2(s) → Al2I6(s)

Identify the oxidation state of H in HCl(aq). Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

When 280. mL of 1.50 × 10-4 mol L-1 hydrochloric acid is added to 135 mL of 1.75 × 10-4 mol L-1 Mg(OH)2, the resulting solution will be ________.

What is the concentration (M) of sodium ions in 4.57 L of a 1.25 mol L-1 Na3P solution?

Determine the oxidation state of Sn in Sn(SO4)2.

Which of the following compounds is soluble in water?

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

How many millilitres of a stock solution of 13.1 mol L-1 would be needed to prepare 0.500 L of 0.500 mol L-1 ?

If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350. mL of solution?

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

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + (g) → N(s) In a particular experiment, 5.50 g samples of each reagent are reacted. What is the theoretical yield of lithium nitride?

Which of the following statements is TRUE?

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

According to the following reaction, what mass of PbCl2 can form from 235 mL of a 0.110 mol L-1 KCl solution? Assume that there is excess Pb(NO3)2. 2KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2KNO3(aq)

What are the required coefficients to properly balance the following chemical reaction? PbS(s) + HBr(aq) → PbBr2(s) + H2S(g)

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How many moles of oxygen 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)

What are the required coefficients to properly balance the following chemical reaction? CH₄(g) + H₂O(g) → CO(g) + H₂(g)

Choose the reaction that represents the combustion of C₆H₁₂O₂.

Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum. Al(s) + I₂(s) → Al₂I₆(s)

Identify the oxidation state of H in HCl(aq). Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)

When 280. mL of 1.50 × 10^-4mol L^-1 hydrochloric acid is added to 135 mL of 1.75 × 10^-4 mol L^-1 Mg(OH)₂, the resulting solution will be ________.

What is the concentration (M) of sodium ions in 4.57 L of a 1.25 mol L^-1 Na₃P solution?

Determine the oxidation state of Sn in Sn(SO₄)₂.

How many millilitres of a stock solution of 13.1 mol L^-1 would be needed to prepare 0.500 L of 0.500 mol L^-1 ?

If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K₃PO₄ in enough water to make 350. mL of solution?

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

According to the following reaction, what mass of PbCl₂ can form from 235 mL of a 0.110 mol L^-1 KCl solution? Assume that there is excess Pb(NO₃)₂. 2KCl(aq) + Pb(NO₃)₂(aq) → PbCl₂(s) + 2KNO₃(aq)

What are the required coefficients to properly balance the following chemical reaction? PbS(s) + HBr(aq) → PbBr₂(s) + H₂S(g)