Question 1

When a solution of Cu(II) chloride, CuCl2 , is added to a solution of potassium sulfide, K2S, a black precipitate of copper sulfide, CuS, forms. Which of the following is the molecular equation for this reaction?

Accepted Answer

A)  CuCl2(aq) + K2S(aq) → CuS(s) + 2 KCl(aq) 
B)  Cu2+(aq) + Cl22-(aq) + K22+(aq) + S2-(aq) → CuS(s) + K22+(aq) + Cl22-(aq) 
C)  Cu2+(aq) + 2 Cl-(aq) + 2 K+(aq) + S2-(aq) → CuS(s) + 2 K+(aq) + 2 Cl- (aq) 
D)  Cu2+(aq) + S2-(aq) → CuS(s)

Question 2

A typical deposit of cholesterol, C27H46O, in an artery has a mass of 3.90 mg. How many molecules of cholesterol are present in this deposit?

Accepted Answer

A)  6.07 × 1021 
B)  6.07 × 1018 
C)  0.00390 
D)  1.65 × 10-22

Question 3

The reaction of nitric acid, HNO3(aq), with calcium carbonate, CaCO3(s) produces calcium nitrate, carbon dioxide, and water. Which of the following is the correct balanced equation for this reaction?

Accepted Answer

A)  HNO3(aq) + CaCO3(s) → CaNO3(aq) + CO2(g) + H2O(l) 
B)  2 HNO3(aq) + CaCO3(s) → CaNO3(aq) + CO2(g) + H2O(l) 
C)  HNO3(aq) + CaCO3(s) → Ca(NO3)2(aq) + CO2(g) + H2O(l) 
D)  2 HNO3(aq) + CaCO3(s) → Ca(NO3)2(aq) + CO2(g) + H2O(l)

Question 4

Lime, CaO, is produced by the reaction CaCO3(s) → CaO(s) + CO2(g). What weight of CO2 is obtained by the decomposition of 38.7 g of CaCO3?

Accepted Answer

A)  15.5 g 
B)  17.0 g 
C)  21.7 g 
D)  23.2 g

Question 5

In an experiment to prepare aspirin, the percent yield was 94.3% G) If the actual yield was 124.3 g, what was the theoretical yield for this experiment?

Accepted Answer

A)  94.3 g 
B)  117 g 
C)  132 g 
D)  234 g

Question 6

Given the reaction 2 HgO(s) → 2 Hg(l) + O2(g). What weight of elemental mercury will be obtained by the decomposition of 94.5 g of HgO?

Accepted Answer

A)  43.8 g 
B)  78.5 g 
C)  87.5 g 
D)  175 g

Question 7

Which of the following compounds has the largest formula weight?

Accepted Answer

A)  aluminum acetate 
B)  calcium acetate 
C)  potassium acetate 
D)  sodium acetate

Question 8

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C2H4(g) + H2O(g) → C2H5OH(l)
If water is present in excess, how many grams of ethanol can be produced from 42.7 g of ethylene?

Accepted Answer

A)  42.7 g 
B)  46.1 g 
C)  70.1 g 
D)  92.2 g

Question 9

The balanced equation for burning octane is: 2 C8H18(g) + 25 O2(g) → 18 H2O(g) + 16 CO2(g). What weight of oxygen is required to completely burn 19.8 g of octane?

Accepted Answer

A)  28.1 g 
B)  34.7 
C)  69.5 
D)  139 g

Question 10

In the industrial synthesis of acetic acid, methanol is reacted with carbon monoxide. The balanced equation for this reaction is: CH3OH(g) + CO(g) → CH3COOH(l)
How many grams of CO(g) are required to produce 16.6 mol of acetic acid?

Accepted Answer

A)  16.6 g 
B)  33.2 g 
C)  465 g 
D)  996 g

Question 11

Which of the following is true of a voltaic cell?

Accepted Answer

A)  The anode is the positive electrode and place where reduction occurs. 
B)  The anode is the positive electrode and place where oxidation occurs. 
C)  The cathode is the positive electrode and place where reduction occurs. 
D)  The cathode is the positive electrode and place where oxidation occurs.

Question 12

Which of the following compounds is insoluble in water?

Accepted Answer

A)  CaCO3 
B)  CaCl2 
C)  Ca(NO3)2 
D)  Ca(C2H3O2)2

Question 13

Which of the following sulfides is soluble in water?

Accepted Answer

A)  Ag2S 
B)  FeS 
C)  K2S 
D)  PbS

Question 14

Which of the following is true of all combustion reactions?

Accepted Answer

A)  They are exothermic. 
B)  They produce carbon dioxide. 
C)  both a and b 
D)  neither a nor b

Question 15

Which of the following definitions of oxidation is generally most useful when dealing with ionic materials?

Accepted Answer

A)  gain of oxygen 
B)  loss of electrons 
C)  loss of hydrogen 
D)  None, these are all equally useful.

Question 16

The term formula weight can be used with respect to which of the following?

Accepted Answer

A)  ionic compounds 
B)  covalent compounds 
C)  both a and b 
D)  neither a nor b

Question 17

A serving of a particular fruit dessert contains 20.0 g of sugar. If all the sugar is sucrose, C12H22O11, how many molecules of sugar are present in this serving?

Accepted Answer

A)  0.0584 
B)  17.1 
C)  3.52 × 1022 
D)  1.03 × 1025

Question 18

How many oxygen atoms are present in 5.20 mol of Al2(SO4)3?

Accepted Answer

A)  62.4 
B)  3.76 × 1025 
C)  9.39 × 1024 
D)  3.13 × 1024

Question 19

Examine the reaction taking place in the beaker in the image. 
-Which of the following might be the product forming in the beaker?

Accepted Answer

A)  KNO3(s) 
B)  AgCl(s) 
C)  Zn(s) 
D)  Pb2+(aq) 
E)  none of the above

Question 20

When solutions of AgNO3 and NaCl react, the balanced molecular equation is: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
How much AgCl is produced when 3.10 g of AgNO3 and 0.600 g of NaCl react?

Accepted Answer

A)  1.47 g 
B)  2.23 g 
C)  2.62 g 
D)  3.70 g

Exam 4: Chemical Reactions

When a solution of Cu(II) chloride, CuCl₂ , is added to a solution of potassium sulfide, K₂S, a black precipitate of copper sulfide, CuS, forms. Which of the following is the molecular equation for this reaction?

A typical deposit of cholesterol, C₂₇H₄₆O, in an artery has a mass of 3.90 mg. How many molecules of cholesterol are present in this deposit?

The reaction of nitric acid, HNO₃(aq) , with calcium carbonate, CaCO₃(s) produces calcium nitrate, carbon dioxide, and water. Which of the following is the correct balanced equation for this reaction?

Lime, CaO, is produced by the reaction CaCO₃(s) → CaO(s) + CO₂(g) . What weight of CO₂ is obtained by the decomposition of 38.7 g of CaCO₃?

In an experiment to prepare aspirin, the percent yield was 94.3% G) If the actual yield was 124.3 g, what was the theoretical yield for this experiment?

Given the reaction 2 HgO(s) → 2 Hg(l) + O₂(g) . What weight of elemental mercury will be obtained by the decomposition of 94.5 g of HgO?

Which of the following compounds has the largest formula weight?

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C₂H₄(g) + H₂O(g) → C₂H₅OH(l) If water is present in excess, how many grams of ethanol can be produced from 42.7 g of ethylene?

The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g) . What weight of oxygen is required to completely burn 19.8 g of octane?

In the industrial synthesis of acetic acid, methanol is reacted with carbon monoxide. The balanced equation for this reaction is: CH₃OH(g) + CO(g) → CH₃COOH(l) How many grams of CO(g) are required to produce 16.6 mol of acetic acid?

Which of the following is true of a voltaic cell?

Which of the following compounds is insoluble in water?

Which of the following sulfides is soluble in water?

Which of the following is true of all combustion reactions?

Which of the following definitions of oxidation is generally most useful when dealing with ionic materials?

The term formula weight can be used with respect to which of the following?

A serving of a particular fruit dessert contains 20.0 g of sugar. If all the sugar is sucrose, C₁₂H₂₂O₁₁, how many molecules of sugar are present in this serving?

How many oxygen atoms are present in 5.20 mol of Al₂(SO₄) ₃?

Examine the reaction taking place in the beaker in the image. -Which of the following might be the product forming in the beaker?

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq) How much AgCl is produced when 3.10 g of AgNO₃ and 0.600 g of NaCl react?

Exam 4: Chemical Reactions

When a solution of Cu(II) chloride, CuCl2 , is added to a solution of potassium sulfide, K2S, a black precipitate of copper sulfide, CuS, forms. Which of the following is the molecular equation for this reaction?

A typical deposit of cholesterol, C27H46O, in an artery has a mass of 3.90 mg. How many molecules of cholesterol are present in this deposit?

The reaction of nitric acid, HNO3(aq) , with calcium carbonate, CaCO3(s) produces calcium nitrate, carbon dioxide, and water. Which of the following is the correct balanced equation for this reaction?

Lime, CaO, is produced by the reaction CaCO3(s) → CaO(s) + CO2(g) . What weight of CO2 is obtained by the decomposition of 38.7 g of CaCO3?

In an experiment to prepare aspirin, the percent yield was 94.3% G) If the actual yield was 124.3 g, what was the theoretical yield for this experiment?

Given the reaction 2 HgO(s) → 2 Hg(l) + O2(g) . What weight of elemental mercury will be obtained by the decomposition of 94.5 g of HgO?

Which of the following compounds has the largest formula weight?

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C2H4(g) + H2O(g) → C2H5OH(l) If water is present in excess, how many grams of ethanol can be produced from 42.7 g of ethylene?

The balanced equation for burning octane is: 2 C8H18(g) + 25 O2(g) → 18 H2O(g) + 16 CO2(g) . What weight of oxygen is required to completely burn 19.8 g of octane?

In the industrial synthesis of acetic acid, methanol is reacted with carbon monoxide. The balanced equation for this reaction is: CH3OH(g) + CO(g) → CH3COOH(l) How many grams of CO(g) are required to produce 16.6 mol of acetic acid?

Which of the following is true of a voltaic cell?

Which of the following compounds is insoluble in water?

Which of the following sulfides is soluble in water?

Which of the following is true of all combustion reactions?

Which of the following definitions of oxidation is generally most useful when dealing with ionic materials?

The term formula weight can be used with respect to which of the following?

A serving of a particular fruit dessert contains 20.0 g of sugar. If all the sugar is sucrose, C12H22O11, how many molecules of sugar are present in this serving?

How many oxygen atoms are present in 5.20 mol of Al2(SO4) 3?

Examine the reaction taking place in the beaker in the image. -Which of the following might be the product forming in the beaker?

When solutions of AgNO3 and NaCl react, the balanced molecular equation is: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) How much AgCl is produced when 3.10 g of AgNO3 and 0.600 g of NaCl react?

When a solution of Cu(II) chloride, CuCl₂ , is added to a solution of potassium sulfide, K₂S, a black precipitate of copper sulfide, CuS, forms. Which of the following is the molecular equation for this reaction?

A typical deposit of cholesterol, C₂₇H₄₆O, in an artery has a mass of 3.90 mg. How many molecules of cholesterol are present in this deposit?

The reaction of nitric acid, HNO₃(aq) , with calcium carbonate, CaCO₃(s) produces calcium nitrate, carbon dioxide, and water. Which of the following is the correct balanced equation for this reaction?

Lime, CaO, is produced by the reaction CaCO₃(s) → CaO(s) + CO₂(g) . What weight of CO₂ is obtained by the decomposition of 38.7 g of CaCO₃?

Given the reaction 2 HgO(s) → 2 Hg(l) + O₂(g) . What weight of elemental mercury will be obtained by the decomposition of 94.5 g of HgO?

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C₂H₄(g) + H₂O(g) → C₂H₅OH(l) If water is present in excess, how many grams of ethanol can be produced from 42.7 g of ethylene?

The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g) . What weight of oxygen is required to completely burn 19.8 g of octane?

In the industrial synthesis of acetic acid, methanol is reacted with carbon monoxide. The balanced equation for this reaction is: CH₃OH(g) + CO(g) → CH₃COOH(l) How many grams of CO(g) are required to produce 16.6 mol of acetic acid?

A serving of a particular fruit dessert contains 20.0 g of sugar. If all the sugar is sucrose, C₁₂H₂₂O₁₁, how many molecules of sugar are present in this serving?

How many oxygen atoms are present in 5.20 mol of Al₂(SO₄) ₃?

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq) How much AgCl is produced when 3.10 g of AgNO₃ and 0.600 g of NaCl react?