Question 1

Describe the difference between complete ionic and net ionic equations.

Accepted Answer

A complete ionic equation shows all of t

Question 2

What is the oxidation number change for the bromine atom in the following unbalanced reduction half-reaction: 
Br O3- (aq)+ H+(aq)→ Br-(aq)+ H2O(l)

Accepted Answer

A) -7 
B) -6 
C) +6 
D) +7 
A) -7 
B) -6 
C) +6 
D) +7

Question 3

The mixing of which pair of reactants will result in a precipitation reaction?

Accepted Answer

A) Ba(NO3)2(aq)+ Na2CO3(aq) 
B) K2SO4(aq)+ Cu(NO3)2(aq) 
C) NaClO4(aq)+ (NH4)2S(aq) 
D) NH4Br(aq)+ NH4I(aq) 
A) Ba(NO3)2(aq)+ Na2CO3(aq) 
B) K2SO4(aq)+ Cu(NO3)2(aq) 
C) NaClO4(aq)+ (NH4)2S(aq) 
D) NH4Br(aq)+ NH4I(aq)

Question 4

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 5

Which one of the following compounds behaves as an acid when dissolved in water?

Accepted Answer

A) RaO 
B) C4H10 
C) HI 
D) RbOH 
A) RaO 
B) C4H10 
C) HI 
D) RbOH

Question 6

Define a salt bridge.

Accepted Answer

A) A pathway,composed of salt water,that ions pass through. 
B) A pathway in which no ions flow. 
C) A pathway between the cathode and anode in which ions are reduced. 
D) A pathway between the cathode and anode in which ions are oxidized. 
E) A pathway through which counterions can flow between the half-cells without the solutions in the half-cell totally mixing. 
A) A pathway,composed of salt water,that ions pass through. 
B) A pathway in which no ions flow. 
C) A pathway between the cathode and anode in which ions are reduced. 
D) A pathway between the cathode and anode in which ions are oxidized. 
E) A pathway through which counterions can flow between the half-cells without the solutions in the half-cell totally mixing.

Question 7

According to the following balanced reaction,how many moles of KO are required to exactly react with 5.44 moles of H2O? 
4KO(s)+ 2H2O(l)→ 4KOH(s)+ O2(g)

Accepted Answer

A) 2.72 moles KO 
B) 16.7 moles KO 
C) 10.9 moles KO 
D) 8.33 moles KO 
E) 4.87 moles KO 
A) 2.72 moles KO 
B) 16.7 moles KO 
C) 10.9 moles KO 
D) 8.33 moles KO 
E) 4.87 moles KO

Question 8

Balance the chemical equation given below,and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25 °C.The density of nitrogen monoxide at $25 ^ { \circ } \mathrm { C }$ is 1.23 g L-1. ________ NH3(g)+ ________ O2(g)? ________ NO(g)+ ________ H2O(l)

Accepted Answer

A) 7.32 L 
B) 11.1 L 
C) 11.5 L 
D) 17.3 L 
A) 7.32 L 
B) 11.1 L 
C) 11.5 L 
D) 17.3 L

Question 9

Which of the following is an acid-base reaction?

Accepted Answer

A) C(s)+ O2(g)→ CO2(g) 
B) 2HClO4(aq)+ Ca(OH)2(aq)→ 2 H2O(l)+ Ca(ClO4)2(aq) 
C) Fe(s)+ 2AgNO3(aq)→ 2Ag(s)+ Fe(NO3)2(aq) 
D) MgSO4(aq)+ Ba(NO3)2(aq)→ Mg(NO3)2(aq)+ BaSO4(s) 
E) None of the above is an acid-base reaction. 
A) C(s)+ O2(g)→ CO2(g) 
B) 2HClO4(aq)+ Ca(OH)2(aq)→ 2 H2O(l)+ Ca(ClO4)2(aq) 
C) Fe(s)+ 2AgNO3(aq)→ 2Ag(s)+ Fe(NO3)2(aq) 
D) MgSO4(aq)+ Ba(NO3)2(aq)→ Mg(NO3)2(aq)+ BaSO4(s) 
E) None of the above is an acid-base reaction.

Question 10

What is the concentration (M)of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in sufficient water to give exactly 230 mL of solution?

Accepted Answer

Question 11

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 12

Balance the following equation:
________ C10H12 + ________ O2 → ________ H2O + ________ CO2

Accepted Answer

C₁₀H₁₂ + 13O₂→

Question 13

Define an electrolyte.

Accepted Answer

A substance that dis

Question 14

What element is undergoing oxidation (if any)in the following reaction? Zn(s)+ 2AgNO3(aq)→ Zn(NO3)2(aq)+ 2Ag(s)

Accepted Answer

A) Zn 
B) N 
C) O 
D) Ag 
E) This is not an oxidation-reduction reaction. 
A) Zn 
B) N 
C) O 
D) Ag 
E) This is not an oxidation-reduction reaction.

Question 15

If 100.mL of 0.400 mol L-1 Na2SO4 is added to 200.mL of 0.600 mol L-1 NaCl,what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive.

Accepted Answer

A) 0.534 mol L-1 
B) 0.667 mol L-1 
C) 1.00 mol L-1 
D) 1.40 mol L-1 
A) 0.534 mol L-1 
B) 0.667 mol L-1 
C) 1.00 mol L-1 
D) 1.40 mol L-1

Question 16

Identify the location of reduction in an electrochemical cell.

Accepted Answer

A) the anode 
B) the cathode 
C) the electrode 
D) the salt bridge 
E) the socket 
A) the anode 
B) the cathode 
C) the electrode 
D) the salt bridge 
E) the socket

Question 17

What is the oxidation number of the sulfur atom in K2SO4 ?

Accepted Answer

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

Question 18

Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution.

Accepted Answer

A) 0.0297 mol L-1 
B) 0.0337 mol L-1 
C) 0.0936 mol L-1 
D) 0.0107 mol L-1 
E) 0.0651 mol L-1 
A) 0.0297 mol L-1 
B) 0.0337 mol L-1 
C) 0.0936 mol L-1 
D) 0.0107 mol L-1 
E) 0.0651 mol L-1

Question 19

According to the following reaction,how many grams of sulfur are formed when 37.4 g of water are formed? 2H2S(g)+ SO2(g)→ 3S(s)+ 2H2O(l)

Accepted Answer

A) 99.8 g S 
B) 66.6 g S 
C) 56.1 g S 
D) 44.4 g S 
E) 14.0 g S 
A) 99.8 g S 
B) 66.6 g S 
C) 56.1 g S 
D) 44.4 g S 
E) 14.0 g S

Question 20

Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: $\mathrm { Ag } ^ { + }$ (aq)+ $\mathrm { Cl } ^ { - }$ (aq)? AgCl(s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion.How many grams of solid NaCl must be added to 25.0 mL of 0.376 mol L-1 $\mathrm { AgNO } _ { 3 }$ solution to completely precipitate the silver?

Accepted Answer

A) 6.22 × 103 g 
B) 0.549 g 
C) 0.161 g 
D) 9.40 × 10-3 g 
E) 1.61 × 10-4 g 
A) 6.22 × 103 g 
B) 0.549 g 
C) 0.161 g 
D) 9.40 × 10-3 g 
E) 1.61 × 10-4 g

Exam 4: Chemical Reactions and Stoichiometry

Describe the difference between complete ionic and net ionic equations.

What is the oxidation number change for the bromine atom in the following unbalanced reduction half-reaction: Br O3- (aq)+ H+(aq)→ Br-(aq)+ H2O(l)

The mixing of which pair of reactants will result in a precipitation reaction?

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?

Which one of the following compounds behaves as an acid when dissolved in water?

Define a salt bridge.

According to the following balanced reaction,how many moles of KO are required to exactly react with 5.44 moles of H2O? 4KO(s)+ 2H2O(l)→ 4KOH(s)+ O2(g)

Which of the following is an acid-base reaction?

What is the concentration (M)of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in sufficient water to give exactly 230 mL of solution?

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)

Balance the following equation: ________ C10H12 + ________ O2 → ________ H2O + ________ CO2

Define an electrolyte.

What element is undergoing oxidation (if any)in the following reaction? Zn(s)+ 2AgNO3(aq)→ Zn(NO3)2(aq)+ 2Ag(s)

If 100.mL of 0.400 mol L-1 Na2SO4 is added to 200.mL of 0.600 mol L-1 NaCl,what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive.

Identify the location of reduction in an electrochemical cell.

What is the oxidation number of the sulfur atom in K2SO4 ?

Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution.

According to the following reaction,how many grams of sulfur are formed when 37.4 g of water are formed? 2H2S(g)+ SO2(g)→ 3S(s)+ 2H2O(l)

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Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Solutions

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Filters

What is the oxidation number change for the bromine atom in the following unbalanced reduction half-reaction: BrO₃^-(aq)+ H⁺(aq)→ Br^-(aq)+ H₂O(l)

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?

According to the following balanced reaction,how many moles of KO are required to exactly react with 5.44 moles of H₂O? 4KO(s)+ 2H₂O(l)→ 4KOH(s)+ O₂(g)

What is the concentration (M)of CH₃OH in a solution prepared by dissolving 16.8 g of CH₃OH in sufficient water to give exactly 230 mL of solution?

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)

Balance the following equation: C₁₀H₁₂ + O₂→ H₂O + CO₂

What element is undergoing oxidation (if any)in the following reaction? Zn(s)+ 2AgNO₃(aq)→ Zn(NO₃)₂(aq)+ 2Ag(s)

If 100.mL of 0.400 mol L^-1 Na₂SO₄ is added to 200.mL of 0.600 mol L^-1 NaCl,what is the concentration of Na⁺ ions in the final solution? Assume that the volumes are additive.

What is the oxidation number of the sulfur atom in K₂SO₄?

Determine the molarity of a solution formed by dissolving 468 mg of MgI₂ in enough water to yield 50.0 mL of solution.

According to the following reaction,how many grams of sulfur are formed when 37.4 g of water are formed? 2H₂S(g)+ SO₂(g)→ 3S(s)+ 2H₂O(l)