Question 1

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

Accepted Answer

Question 2

Given the following standard reduction potentials,   calculate the formation constant of Ag(NH3)2+ at 25°C.

Accepted Answer

A) 6.1 $\times$ 10-15 
B) 1.5 $\times$ 10-13 
C) 6.9 $\times$ 1012 
D) 1.6 $\times$ 1014 
E) None of these 
A) 6.1 $\times$ 10-15 
B) 1.5 $\times$ 10-13 
C) 6.9 $\times$ 1012 
D) 1.6 $\times$ 1014 
E) None of these

Question 3

Calculate the cell voltage for the following reaction: Cu2+ (0.010 M)+ H2(1 atm)$\to$ Cu(s)+ 2H+( pH = 7.0)

Accepted Answer

A) 0.19 V 
B) -0.01 V 
C) 0.34 V 
D) 0.69 V 
E) 0.49 V 
A) 0.19 V 
B) -0.01 V 
C) 0.34 V 
D) 0.69 V 
E) 0.49 V

Question 4

Calculate E°cell for the following reaction: 2Fe2+(aq)+ Cd2+(aq)$\to$ 2Fe3+(aq)+ Cd(s)

Accepted Answer

A) -0.37 V 
B) 0.37 V 
C) -1.17 V 
D) 1.17 V 
E) None of these. 
A) -0.37 V 
B) 0.37 V 
C) -1.17 V 
D) 1.17 V 
E) None of these.

Question 5

How many moles of H2 are produced by 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 $\times$ 102 s?

Accepted Answer

The answer of How many moles of H2 are produced...

Question 6

How many minutes would be required to electroplate 25.0 grams of chromium by passing a constant current of 4.80 amperes through a solution containing CrCl3?

Accepted Answer

A) 483 min 
B) 161 min 
C) 322 min 
D) 2.01 $\times$ 104 min 
E) 1.11 $\times$ 104 min 
A) 483 min 
B) 161 min 
C) 322 min 
D) 2.01 $\times$ 104 min 
E) 1.11 $\times$ 104 min

Question 7

Consider the following standard reduction potentials in acid solution:   The strongest oxidizing agent among those shown above is

Accepted Answer

A) Fe3+. 
B) Fe2+. 
C) Br-. 
D) Al3+. 
E) Al. 
A) Fe3+. 
B) Fe2+. 
C) Br-. 
D) Al3+. 
E) Al.

Question 8

Determine the equilibrium constant (Keq)at 25°C for the reaction Cl2(g)+ 2Br- (aq)    
2Cl- (aq)+ Br2(l)

Accepted Answer

A) 1.5 $\times$ 10-10 
B) 6.3 $\times$ 109 
C) 1.3 $\times$ 1041 
D) 8.1 $\times$ 104 
E) 9.8 
A) 1.5 $\times$ 10-10 
B) 6.3 $\times$ 109 
C) 1.3 $\times$ 1041 
D) 8.1 $\times$ 104 
E) 9.8

Question 9

Suppose the reaction Pb(s)+ 2H+(aq)$\to$Pb2+(aq)+ H2(g)is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II)ions that causes this reaction to be at equilibrium is

Accepted Answer

A) 2.5 M 
B) 1.6 $\times$ 10-2 M 
C) 2.5 $\times$ 10-4 M 
D) 1.6 $\times$ 10-6 M 
E) 0.40 M 
A) 2.5 M 
B) 1.6 $\times$ 10-2 M 
C) 2.5 $\times$ 10-4 M 
D) 1.6 $\times$ 10-6 M 
E) 0.40 M

Question 10

What current is needed to deposit 0.500 g of chromium metal from a solution of Cr3+ in a period of 1.00 hr?

Accepted Answer

Question 11

Given the following notation for an electrochemical cell Pt(s)| H2(g)| H+(aq)|| Ag+(aq)| Ag(s)
What is the balanced overall (net)cell reaction?

Accepted Answer

A) 2H+(aq)+ 2Ag+(aq)$\to$ H2(g)+ 2Ag(s) 
B) H2(g)+ 2Ag(s)$\to$ H+(aq)+ 2Ag+(aq) 
C) 2H+(aq)+ 2Ag(s)$\to$ H2(g)+ 2Ag+(aq) 
D) H2(g)+ Ag+(aq)$\to$H+(aq)+ Ag(s) 
E) H2(g)+ 2Ag+(aq)$\to$ 2H+(aq)+ 2Ag(s) 
A) 2H+(aq)+ 2Ag+(aq)$\to$ H2(g)+ 2Ag(s) 
B) H2(g)+ 2Ag(s)$\to$ H+(aq)+ 2Ag+(aq) 
C) 2H+(aq)+ 2Ag(s)$\to$ H2(g)+ 2Ag+(aq) 
D) H2(g)+ Ag+(aq)$\to$H+(aq)+ Ag(s) 
E) H2(g)+ 2Ag+(aq)$\to$ 2H+(aq)+ 2Ag(s)

Question 12

Consider the following standard reduction potentials in acid solution:   The weakest reducing agent listed above is

Accepted Answer

A) Cr3+. 
B) Cr. 
C) Mn2+. 
D) Co. 
E) MnO4-. 
A) Cr3+. 
B) Cr. 
C) Mn2+. 
D) Co. 
E) MnO4-.

Question 13

Consider an electrochemical cell involving the overall reaction 2AgBr(s)+ Pb(s)$\to$ Pb2+ + 2Ag(s)+ 2Br-
 Each half-reaction is carried out in a separate compartment. The anion included in the lead half-cell is NO3-. The cation in the silver half-cell is K+. The two half-cells are connected by a KNO3 salt bridge. If [Pb2+] = 1.0 M, what concentration of Br- ion will produce a cell emf of 0.25 V at 298 K?
Given: AgBr(s)+ e- $\to$ Ag + Br-, E° = +0.07 V.

Accepted Answer

A) 0.02 M 
B) 0.14 M 
C) 0.38 M 
D) 1.0 M 
E) 7.0 M 
A) 0.02 M 
B) 0.14 M 
C) 0.38 M 
D) 1.0 M 
E) 7.0 M

Question 14

Given the following standard reduction potentials in acid solution   write the formula of the strongest reducing agent.

Accepted Answer

The answer of Given the following standard reduction potentials in...

Question 15

Calculate the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution. 2H2O + 2Cl- (1.0 M)$\to$  H2(1 atm)+ Cl2(1 atm)+ 2OH- (1 $\times$ 10-7 M)

Accepted Answer

A) 2.19 V 
B) 1.78 V 
C) 0.41 V 
D) -0.41 V 
E) -1.78 V 
A) 2.19 V 
B) 1.78 V 
C) 0.41 V 
D) -0.41 V 
E) -1.78 V

Question 16

When a solution of a certain gadolinium salt is electrolyzed with a current of 1.0 A for 2.0 h, 0.025 mol of Gd metal forms. Calculate the charge on the gadolinium ion in the salt.

Accepted Answer

The answer of When a solution of a certain gadolinium...

Question 17

Which one of the following reactions must be carried out in an electrolytic cell rather than in a galvanic cell?

Accepted Answer

A) Zn2+ + Ca $\to$  Zn + Ca2+ 
B) Al3+ + 3Br- $\to$  Al + (3/2)Br2 
C) 2Al + 3Fe2+$\to$ 2Al3+ + 3Fe 
D) H2 + I2(s)$\to$ 2H+ + 2I- 
A) Zn2+ + Ca $\to$  Zn + Ca2+ 
B) Al3+ + 3Br- $\to$  Al + (3/2)Br2 
C) 2Al + 3Fe2+$\to$ 2Al3+ + 3Fe 
D) H2 + I2(s)$\to$ 2H+ + 2I-

Question 18

How many coulombs of charge are required to cause reduction of 0.25 mole of Cu2+ to Cu?

Accepted Answer

A) 0.25 C 
B) 0.50 C 
C) 1.2 $\times$ 104 C 
D) 2.4 $\times$ 104 C 
E) 4.8 $\times$ 104 C 
A) 0.25 C 
B) 0.50 C 
C) 1.2 $\times$ 104 C 
D) 2.4 $\times$ 104 C 
E) 4.8 $\times$ 104 C

Question 19

Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced with the set of smallest whole-number coefficients? H2O + MnO4- + I- $\to$ MnO2 + IO3- (basic solution)

Accepted Answer

A) 1 
B) 2 
C) 4 
D) 10 
E) None of these. 
A) 1 
B) 2 
C) 4 
D) 10 
E) None of these.

Question 20

Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced using the set of smallest whole-number coefficients? MnO4- + SO32- $\to$ Mn2+ + SO42- (acidic solution)

Accepted Answer

A) 3 
B) 4 
C) 5 
D) 8 
E) None of these. 
A) 3 
B) 4 
C) 5 
D) 8 
E) None of these.

Exam 19: Electrochemistry

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

Given the following standard reduction potentials, calculate the formation constant of Ag(NH3)2+ at 25°C.

Calculate the cell voltage for the following reaction: Cu2+ (0.010 M)+ H2(1 atm) →\to→ Cu(s)+ 2H+( pH = 7.0)

Calculate E°cell for the following reaction: 2Fe2+(aq)+ Cd2+(aq) →\to→ 2Fe3+(aq)+ Cd(s)

How many moles of H2 are produced by 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 ×\times× 102 s?

How many minutes would be required to electroplate 25.0 grams of chromium by passing a constant current of 4.80 amperes through a solution containing CrCl3?

Consider the following standard reduction potentials in acid solution: The strongest oxidizing agent among those shown above is

Determine the equilibrium constant (Keq)at 25°C for the reaction Cl2(g)+ 2Br- (aq) 2Cl- (aq)+ Br2(l)

Suppose the reaction Pb(s)+ 2H+(aq) →\to→ Pb2+(aq)+ H2(g)is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II)ions that causes this reaction to be at equilibrium is

What current is needed to deposit 0.500 g of chromium metal from a solution of Cr3+ in a period of 1.00 hr?

Given the following notation for an electrochemical cell Pt(s)| H2(g)| H+(aq)|| Ag+(aq)| Ag(s) What is the balanced overall (net)cell reaction?

Consider the following standard reduction potentials in acid solution: The weakest reducing agent listed above is

Given the following standard reduction potentials in acid solution write the formula of the strongest reducing agent.

Calculate the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution. 2H2O + 2Cl- (1.0 M) →\to→ H2(1 atm)+ Cl2(1 atm)+ 2OH- (1 ×\times× 10-7 M)

When a solution of a certain gadolinium salt is electrolyzed with a current of 1.0 A for 2.0 h, 0.025 mol of Gd metal forms. Calculate the charge on the gadolinium ion in the salt.

Which one of the following reactions must be carried out in an electrolytic cell rather than in a galvanic cell?

How many coulombs of charge are required to cause reduction of 0.25 mole of Cu2+ to Cu?

Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced with the set of smallest whole-number coefficients? H2O + MnO4- + I- →\to→ MnO2 + IO3- (basic solution)

Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced using the set of smallest whole-number coefficients? MnO4- + SO32- →\to→ Mn2+ + SO42- (acidic solution)

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Filters

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

Given the following standard reduction potentials, calculate the formation constant of Ag(NH₃)₂⁺at 25°C.

Calculate the cell voltage for the following reaction: Cu²⁺ (0.010 M)+ H₂(1 atm) $\to$ Cu(s)+ 2H⁺( pH = 7.0)

Calculate E°_cell for the following reaction: 2Fe²⁺(aq)+ Cd²⁺(aq) $\to$ 2Fe³⁺(aq)+ Cd(s)

How many moles of H₂ are producedby 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 $\times$ 10² s?

How many minutes would be required to electroplate 25.0 grams of chromium by passing a constant current of 4.80 amperes through a solution containing CrCl₃?

Determine the equilibrium constant (K_eq)at 25°C for the reaction Cl₂(g)+ 2Br^-(aq) 2Cl^-(aq)+ Br₂(l)

Suppose the reaction Pb(s)+ 2H⁺(aq) $\to$ Pb²⁺(aq)+ H₂(g)is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II)ions that causes this reaction to be at equilibrium is

What current is needed to deposit 0.500 g of chromium metal from a solution of Cr³⁺ in a period of 1.00 hr?

Given the following notation for an electrochemical cell Pt(s)| H₂(g)| H⁺(aq)|| Ag⁺(aq)| Ag(s) What is the balanced overall (net)cell reaction?

Calculate the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution. 2H₂O + 2Cl^-(1.0 M) $\to$ H₂(1 atm)+ Cl₂(1 atm)+ 2OH^-(1 $\times$ 10^-7 M)

How many coulombs of charge are required to cause reduction of 0.25 mole of Cu²⁺ to Cu?

Complete and balance the following redox equation. What is the coefficient of H₂O when the equation is balanced with the set of smallest whole-number coefficients? H₂O + MnO₄^- + I^- $\to$ MnO₂ + IO₃^- (basic solution)

Complete and balance the following redox equation. What is the coefficient of H₂O when the equation is balanced using the set of smallest whole-number coefficients? MnO₄^- + SO₃^2- $\to$ Mn²⁺ + SO₄^2- (acidic solution)