Question 1

Consider the reaction Hg2+(aq)+ Hg(l)   Hg22+(aq). Find the equilibrium constant for this reaction at 25°C.

Accepted Answer

A) 2 $\times$ 101 
B) 6 $\times$ 1059 
C) 4 $\times$ 10-3 
D) 7 $\times$ 10-2 
E) 2 $\times$ 102 
A) 2 $\times$ 101 
B) 6 $\times$ 1059 
C) 4 $\times$ 10-3 
D) 7 $\times$ 10-2 
E) 2 $\times$ 102

Question 2

Aluminum metal is formed by the electrolysis of Al2O3 in molten cryolite. How many grams of Al are produced when 6.50 $\times$ 103 C pass through the cell?

Accepted Answer

The answer of Aluminum metal is formed by the electrolysis...

Question 3

Aluminum metal is formed by the electrolysis of Al2O3 in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

Accepted Answer

Question 4

Consider the reaction Fe + Sn2+(1 $\times$ 10-3 M)$\to$ Fe2+(1.0 M)+ Sn. Sketch a diagram of such a cell. Be sure to label the anode and cathode, and show the direction of electron flow in the external circuit. Write the half-reactions occurring at the electrodes.

Accepted Answer

Fe | Fe²⁺(1.0 M)||

Question 5

Which element is associated with the term "galvanized"?

Accepted Answer

A) Ga 
B) Zn 
C) Cd 
D) Hg 
E) Pb 
A) Ga 
B) Zn 
C) Cd 
D) Hg 
E) Pb

Question 6

Complete and balance the following redox equation using the set of smallest whole-numbers coefficients. What is the sum of the coefficients? HI + HNO3 $\to$ I2 + NO (acidic solution)

Accepted Answer

A) 5 
B) 7 
C) 14 
D) 17 
E) None of these. 
A) 5 
B) 7 
C) 14 
D) 17 
E) None of these.

Question 7

Gold can be electrochemically "plated" onto a less expensive metal by submerging the object in a solution of gold(III)and applying an electric current to drive the following half-reaction:
Au3+ + 3e- $\to$  Au(s)
How many grams of gold will be formed if a current of 2.37 A is applied for 71 minutes?

Accepted Answer

The answer of Gold can be electrochemically "plated" onto a...

Question 8

Which of these metals will be oxidized in hydrochloric acid under standard conditions at 25°C?

Accepted Answer

A) Ag 
B) Au 
C) Hg 
D) Cu 
E) Zn 
A) Ag 
B) Au 
C) Hg 
D) Cu 
E) Zn

Question 9

Consider the reaction 2Fe3+(aq)+ Fe(s)    3Fe2+(aq). Find the equilibrium constant for this reaction at 25°C.

Accepted Answer

A) 1 $\times$ 1011 
B) 8 $\times$ 1040 
C) 3 $\times$ 1020 
D) 7 $\times$ 10-12 
E) 1 $\times$ 10-41 
A) 1 $\times$ 1011 
B) 8 $\times$ 1040 
C) 3 $\times$ 1020 
D) 7 $\times$ 10-12 
E) 1 $\times$ 10-41

Question 10

Will H2(g)form when Ag is placed in 1.0 M HCl?

Accepted Answer

Question 11

Find the emf of the cell described by the cell diagram Fe | Fe2+ (1.500M)|| Au3+ (0.00400M)| Au

Accepted Answer

A) 1.99 V 
B) 1.89 V 
C) 1.94 V 
D) 1.66 V 
E) 1.91 V 
A) 1.99 V 
B) 1.89 V 
C) 1.94 V 
D) 1.66 V 
E) 1.91 V

Question 12

Which statement is true for a spontaneous redox reaction carried out at standard-state conditions?

Accepted Answer

A) E°red is always negative. 
B) E°cell is always positive. 
C) E°ox is always positive. 
D) E°red is always positive. 
A) E°red is always negative. 
B) E°cell is always positive. 
C) E°ox is always positive. 
D) E°red is always positive.

Question 13

Iron objects such as storage tanks and underground pipelines can be protected from corrosion by connecting them through a wire to a piece of

Accepted Answer

A) Pb 
B) Ag 
C) Sn 
D) Mg 
E) Cu 
A) Pb 
B) Ag 
C) Sn 
D) Mg 
E) Cu

Question 14

Calculate the cell emf for the following reaction: Cu2+(0.10 M)+ H2(1 atm)$\to$ Cu(s)+ 2H+(pH = 3.00)

Accepted Answer

A) 0.49 V 
B) 0.19 V 
C) 0.15 V 
D) 0.40 V 
E) -0.34 V 
A) 0.49 V 
B) 0.19 V 
C) 0.15 V 
D) 0.40 V 
E) -0.34 V

Question 15

Complete and balance the following redox reaction under basic conditions:
PO33-(aq)+ MnO4-(aq)$\to$  PO43-(aq)+ MnO2(s)

Accepted Answer

3PO₃^3-(a

Question 16

Which of these metals will not reduce water to hydrogen in basic solution under standard conditions?

Accepted Answer

A) Cd 
B) Sr 
C) Mg 
D) Ba 
E) K 
A) Cd 
B) Sr 
C) Mg 
D) Ba 
E) K

Question 17

Many different ways have been proposed to make batteries.One cell is set up with copper and lead electrodes in contact with CuSO4(aq)and Pb(NO3)2 (aq), respectively.If the Pb2+ and Cu2+ concentrations are each 1.0 M, what is the overall cell potential?

Accepted Answer

Question 18

In the following half equation, which is the oxidizing agent? NO3-(aq)+ 4H+(aq)+ 3e- $\to$ NO(g)+ 2H2O

Accepted Answer

A) NO3- 
B) H+ 
C) e- 
D) NO 
E) H2O 
A) NO3- 
B) H+ 
C) e- 
D) NO 
E) H2O

Exam 19: Electrochemistry

Consider the reaction Hg2+(aq)+ Hg(l) Hg22+(aq). Find the equilibrium constant for this reaction at 25°C.

Aluminum metal is formed by the electrolysis of Al2O3 in molten cryolite. How many grams of Al are produced when 6.50 ×\times× 103 C pass through the cell?

Aluminum metal is formed by the electrolysis of Al2O3 in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

Consider the reaction Fe + Sn2+(1 ×\times× 10-3 M) →\to→ Fe2+(1.0 M)+ Sn. Sketch a diagram of such a cell. Be sure to label the anode and cathode, and show the direction of electron flow in the external circuit. Write the half-reactions occurring at the electrodes.

Which element is associated with the term "galvanized"?

Complete and balance the following redox equation using the set of smallest whole-numbers coefficients. What is the sum of the coefficients? HI + HNO3 →\to→ I2 + NO (acidic solution)

Which of these metals will be oxidized in hydrochloric acid under standard conditions at 25°C?

Consider the reaction 2Fe3+(aq)+ Fe(s) 3Fe2+(aq). Find the equilibrium constant for this reaction at 25°C.

Will H2(g)form when Ag is placed in 1.0 M HCl?

Find the emf of the cell described by the cell diagram Fe | Fe2+ (1.500M)|| Au3+ (0.00400M)| Au

Which statement is true for a spontaneous redox reaction carried out at standard-state conditions?

Iron objects such as storage tanks and underground pipelines can be protected from corrosion by connecting them through a wire to a piece of

Calculate the cell emf for the following reaction: Cu2+(0.10 M)+ H2(1 atm) →\to→ Cu(s)+ 2H+(pH = 3.00)

Complete and balance the following redox reaction under basic conditions: PO33-(aq)+ MnO4-(aq) →\to→ PO43-(aq)+ MnO2(s)

Which of these metals will not reduce water to hydrogen in basic solution under standard conditions?

Many different ways have been proposed to make batteries.One cell is set up with copper and lead electrodes in contact with CuSO4(aq)and Pb(NO3)2 (aq), respectively.If the Pb2+ and Cu2+ concentrations are each 1.0 M, what is the overall cell potential?

In the following half equation, which is the oxidizing agent? NO3-(aq)+ 4H+(aq)+ 3e- →\to→ NO(g)+ 2H2O

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

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Consider the reaction Hg²⁺(aq)+ Hg(l) Hg₂²⁺(aq). Find the equilibrium constant for this reaction at 25°C.

Aluminum metal is formed by the electrolysis of Al₂O₃in molten cryolite. How many grams of Al are produced when 6.50 $\times$ 10³ C pass through the cell?

Aluminum metal is formed by the electrolysis of Al₂O₃in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

Consider the reaction Fe + Sn²⁺(1 $\times$ 10^-3 M) $\to$ Fe²⁺(1.0 M)+ Sn. Sketch a diagram of such a cell. Be sure to label the anode and cathode, and show the direction of electron flow in the external circuit. Write the half-reactions occurring at the electrodes.

Complete and balance the following redox equation using the set of smallest whole-numbers coefficients. What is the sum of the coefficients? HI + HNO₃ $\to$ I₂ + NO (acidic solution)

Consider the reaction 2Fe³⁺(aq)+ Fe(s) 3Fe²⁺(aq). Find the equilibrium constant for this reaction at 25°C.

Will H₂(g)form when Ag is placed in 1.0 M HCl?

Find the emf of the cell described by the cell diagram Fe | Fe²⁺ (1.500M)|| Au³⁺ (0.00400M)| Au

Calculate the cell emf for the following reaction: Cu²⁺(0.10 M)+ H₂(1 atm) $\to$ Cu(s)+ 2H⁺(pH = 3.00)

Complete and balance the following redox reaction under basic conditions: PO₃^3-(aq)+ MnO₄^-(aq) $\to$ PO₄^3-(aq)+ MnO₂(s)

Many different ways have been proposed to make batteries.One cell is set up with copper and lead electrodes in contact with CuSO₄(aq)and Pb(NO₃)₂ (aq), respectively.If the Pb²⁺ and Cu²⁺concentrations are each 1.0 M, what is the overall cell potential?

In the following half equation, which is the oxidizing agent? NO₃^-(aq)+ 4H⁺(aq)+ 3e^- $\to$ NO(g)+ 2H₂O