Question 1

The following has a potential of 0.34 V. 2 is 1.0 atm,then E° for the half-reaction   is _____. A)  0.17 V B)  -0.17 V C)  0.34 V D)  -0.34 V E)  None of these" class="answers-bank-image d-inline" rel="preload" > If the concentrations of each of the ions is 1.0 M and the pressure of H2 is 1.0 atm,then E° for the half-reaction 2 is 1.0 atm,then E° for the half-reaction   is _____. A)  0.17 V B)  -0.17 V C)  0.34 V D)  -0.34 V E)  None of these" class="answers-bank-image d-inline" rel="preload" > is _____.

Accepted Answer

A)   0.17 V
B)   -0.17 V
C)   0.34 V
D)   -0.34 V
E)   None of theseF) A) and B)
G) All of the above

Question 2

Calculate the equilibrium constant for the following reaction at 25 °C, 2 IO3-(aq) + 5 Hg( 3-(aq) + 5 Hg(   ) + 12 H+(aq) → I2(s) + 5 Hg2+(aq) + 6 H2O(   )  The standard reduction potentials are as follows: IO3-(aq) + 6 H+(aq) + 5 e- → I2(s) + 3 H2O(   )  E° = +1.20 V Hg2+(aq) + 2 e- → Hg(   )  E° = +0.86 V A)  3 × 10-58 B)  6 × 105 C)  3 × 1011 D)  6 × 1028 E)  3 × 1057" class="answers-bank-image d-inline" rel="preload" > ) + 12 H+(aq) → I2(s) + 5 Hg2+(aq) + 6 H2O( 3-(aq) + 5 Hg(   ) + 12 H+(aq) → I2(s) + 5 Hg2+(aq) + 6 H2O(   )  The standard reduction potentials are as follows: IO3-(aq) + 6 H+(aq) + 5 e- → I2(s) + 3 H2O(   )  E° = +1.20 V Hg2+(aq) + 2 e- → Hg(   )  E° = +0.86 V A)  3 × 10-58 B)  6 × 105 C)  3 × 1011 D)  6 × 1028 E)  3 × 1057" class="answers-bank-image d-inline" rel="preload" > ) 
The standard reduction potentials are as follows:
IO3-(aq) + 6 H+(aq) + 5 e- → I2(s) + 3 H2O( 3-(aq) + 5 Hg(   ) + 12 H+(aq) → I2(s) + 5 Hg2+(aq) + 6 H2O(   )  The standard reduction potentials are as follows: IO3-(aq) + 6 H+(aq) + 5 e- → I2(s) + 3 H2O(   )  E° = +1.20 V Hg2+(aq) + 2 e- → Hg(   )  E° = +0.86 V A)  3 × 10-58 B)  6 × 105 C)  3 × 1011 D)  6 × 1028 E)  3 × 1057" class="answers-bank-image d-inline" rel="preload" > ) 
E° = +1.20 V
Hg2+(aq) + 2 e- → Hg( 3-(aq) + 5 Hg(   ) + 12 H+(aq) → I2(s) + 5 Hg2+(aq) + 6 H2O(   )  The standard reduction potentials are as follows: IO3-(aq) + 6 H+(aq) + 5 e- → I2(s) + 3 H2O(   )  E° = +1.20 V Hg2+(aq) + 2 e- → Hg(   )  E° = +0.86 V A)  3 × 10-58 B)  6 × 105 C)  3 × 1011 D)  6 × 1028 E)  3 × 1057" class="answers-bank-image d-inline" rel="preload" > ) 
E° = +0.86 V

Accepted Answer

A)   3 × 10-58
B)   6 × 105
C)   3 × 1011
D)   6 × 1028
E)   3 × 1057F) A) and B)
G) All of the above

Question 3

Calculate the standard cell potential ( 2+(aq) → 2 Ag+(aq) + Co(s) . The standard reduction potentials are as follows: Ag+(aq) + e−→ Ag(s)  E° = 0.8 V Co2+(aq) +2 e−→ Co(s)  E° = -0.277 V A)  -1.077 V B)  1.077 V C)  -1.877 V D)  1.877 V E)  1.323 V" class="answers-bank-image d-inline" rel="preload" > ) for the reaction 2 Ag(s) + Co2+(aq) → 2 Ag+(aq) + Co(s) . The standard reduction potentials are as follows:
Ag+(aq) + e−→ Ag(s) 
E° = 0.8 V
Co2+(aq) +2 e−→ Co(s) 
E° = -0.277 V

Accepted Answer

A)   -1.077 V
B)   1.077 V
C)   -1.877 V
D)   1.877 V
E)   1.323 VF) C) and D)
G) None of the above

Question 4

Calculate Ecell for the following electrochemical cell at 25 °C Pt(s) | H2(g,1.00 atm) | H+(aq,1.00 M) || Sn2+(aq,0.350 M) ,Sn4+(aq,0.020 M) | Pt(s) 
The standard reduction potentials are as follows:
Sn4+(aq) + 2 e- → Sn2+(s) 
E° = +0.15 V
2 H+(aq) + 2 e- → H2(g) 
E° = 0.00 V

Accepted Answer

A)   -0.19 V
B)   +0.08 V
C)   +0.11 V
D)   +0.19 V
E)   +0.22 VF) A) and B)
G) C) and E)

Question 5

For the following cell reaction,the standard cell potential is 1.34 V.To determine the cell potential at nonstandard conditions,what is the value that should be used for n in the Nernst equation?

Accepted Answer

A)   8
B)   10
C)   5
D)   2
E)   6F) A) and D)
G) B) and C)

Question 6

When the given oxidation-reduction reaction in an acidic solution is balanced,what is the lowest whole-number coefficient for H+,and on which side of the balanced equation should it appear? MnO4-(aq) + Br-(aq) → Mn2+(aq) + Br2(l)

Accepted Answer

A)   1; reactant side
B)   2; product side
C)   8; reactant side
D)   16; reactant side
E)   4; product sideF) A) and B)
G) C) and E)

Question 7

Which of the following reactions will require the use of an inert electrode when used in a voltaic cell?

Accepted Answer

A)   Co(s) + 2 Ag+(aq) → 2 Ag(s) + Co2+(aq) 
B)   3 Ni(s) + 2 Au3+(aq) → 3 Ni2+ + 2 Au(s) 
C)   Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2 Ag(s) 
D)   Zn(s) + 2 MnO2(s) + 2 NH4+(aq) → Zn2+(aq) + Mn2O3(s) + 2 NH3(aq) + H2O(l) 
E)   3 Zn2+(aq) + 2 Al(s) → 3 Zn(s) + 2 Al3+(aq) F) C) and D)
G) A) and B)

Question 8

Which of the following statements concerning voltaic cells is not true?

Accepted Answer

A)   A salt bridge allows cations and anions to move between half-cells.
B)   Electrons flow from a cathode to an anode in the external circuit.
C)   Oxidation occurs at an anode.
D)   A voltaic cell can be used as a source of energy.
E)   A voltaic cell consists of two half-cells.F) None of the above
G) All of the above

Question 9

Primary batteries are also called storage batteries or rechargeable batteries.

Accepted Answer

A) True 
 B)False

Question 10

In the context of the diagram given below,which of the following statements is true concerning half-cell II? 2+] decreases with time,and [K+] increases with time. B)  [Cu2+] increases with time,and [K+] increases with time. C)  [Cu2+] decreases with time,and [K+] decreases with time. D)  [Cu2+] decreases with time,and [SO42-] decreases with time. E)  [Cu2+] increases with time,and [SO42-] increases with time." class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   [Cu2+] decreases with time,and [K+] increases with time.
B)   [Cu2+] increases with time,and [K+] increases with time.
C)   [Cu2+] decreases with time,and [K+] decreases with time.
D)   [Cu2+] decreases with time,and [SO42-] decreases with time.
E)   [Cu2+] increases with time,and [SO42-] increases with time.F) B) and C)
G) A) and E)

Question 11

Write a balanced half-reaction for the reduction of CrO42-(aq) to Cr(OH) 3(s) in a basic solution.

Accepted Answer

A)   CrO42-(aq) + 3 OH-(aq) + 3 e- → Cr(OH) 3(s) + 2 O2(g) 
B)   CrO42-(aq) + 3 H+(aq) + 3 e- → Cr(OH) 3(s) 
C)   CrO42-(aq) + 3 H+(aq) → Cr(OH) 3(s) + 2 e-
D)   CrO42-(aq) + 4 H2O( 42-(aq) to Cr(OH) 3(s) in a basic solution. 
A)   CrO42-(aq) + 3 OH-(aq) + 3 e- → Cr(OH) 3(s) + 2 O2(g)  
B)   CrO42-(aq) + 3 H+(aq) + 3 e- → Cr(OH) 3(s)  
C)   CrO42-(aq) + 3 H+(aq) → Cr(OH) 3(s) + 2 e- 
D)   CrO42-(aq) + 4 H2O(   ) + 3 e- → Cr(OH) 3(s) + 5 OH-(aq)  
E)   CrO42-(aq) + 3 OH-(aq) → Cr(OH) 3(s) + 2 O2(g) " class="answers-bank-image d-inline" rel="preload" > ) + 3 e- → Cr(OH) 3(s) + 5 OH-(aq) 
E)   CrO42-(aq) + 3 OH-(aq) → Cr(OH) 3(s) + 2 O2(g) F) A) and E)
G) A) and B)

Question 12

Which of the following overall chemical equations is responsible for generating electricity in fuel cells used in NASA's Space Shuttle programs?

Accepted Answer

A)   Fe2O3(s) + Al(s) → Fe(s) + Al2O3(s) 
B)   Pb(s) + PbO2(s) + 2 H2SO4(aq) → 2 PbSO4(s) + 2 H2O( 2O3(s) + Al(s) → Fe(s) + Al2O3(s)  
B)   Pb(s) + PbO2(s) + 2 H2SO4(aq) → 2 PbSO4(s) + 2 H2O(   )  
C)   2 NiO(OH) (s) + Cd(s) + H2O(   ) → 2 Ni(OH) 2(s) + Cd(OH) 2(s)  
D)   2 H2(g) + O2(g) → 2 H2O(   )  
E)   N2H4(   ) + O2(g) → N2(g) + 2 H2O(   ) " class="answers-bank-image d-inline" rel="preload" > ) 
C)   2 NiO(OH) (s) + Cd(s) + H2O( 2O3(s) + Al(s) → Fe(s) + Al2O3(s)  
B)   Pb(s) + PbO2(s) + 2 H2SO4(aq) → 2 PbSO4(s) + 2 H2O(   )  
C)   2 NiO(OH) (s) + Cd(s) + H2O(   ) → 2 Ni(OH) 2(s) + Cd(OH) 2(s)  
D)   2 H2(g) + O2(g) → 2 H2O(   )  
E)   N2H4(   ) + O2(g) → N2(g) + 2 H2O(   ) " class="answers-bank-image d-inline" rel="preload" > ) → 2 Ni(OH) 2(s) + Cd(OH) 2(s) 
D)   2 H2(g) + O2(g) → 2 H2O( 2O3(s) + Al(s) → Fe(s) + Al2O3(s)  
B)   Pb(s) + PbO2(s) + 2 H2SO4(aq) → 2 PbSO4(s) + 2 H2O(   )  
C)   2 NiO(OH) (s) + Cd(s) + H2O(   ) → 2 Ni(OH) 2(s) + Cd(OH) 2(s)  
D)   2 H2(g) + O2(g) → 2 H2O(   )  
E)   N2H4(   ) + O2(g) → N2(g) + 2 H2O(   ) " class="answers-bank-image d-inline" rel="preload" > ) 
E)   N2H4( 2O3(s) + Al(s) → Fe(s) + Al2O3(s)  
B)   Pb(s) + PbO2(s) + 2 H2SO4(aq) → 2 PbSO4(s) + 2 H2O(   )  
C)   2 NiO(OH) (s) + Cd(s) + H2O(   ) → 2 Ni(OH) 2(s) + Cd(OH) 2(s)  
D)   2 H2(g) + O2(g) → 2 H2O(   )  
E)   N2H4(   ) + O2(g) → N2(g) + 2 H2O(   ) " class="answers-bank-image d-inline" rel="preload" > ) + O2(g) → N2(g) + 2 H2O( 2O3(s) + Al(s) → Fe(s) + Al2O3(s)  
B)   Pb(s) + PbO2(s) + 2 H2SO4(aq) → 2 PbSO4(s) + 2 H2O(   )  
C)   2 NiO(OH) (s) + Cd(s) + H2O(   ) → 2 Ni(OH) 2(s) + Cd(OH) 2(s)  
D)   2 H2(g) + O2(g) → 2 H2O(   )  
E)   N2H4(   ) + O2(g) → N2(g) + 2 H2O(   ) " class="answers-bank-image d-inline" rel="preload" > ) F) C) and E)
G) None of the above

Question 13

Which of the following statements is true for the following reaction,assuming the given reaction proceeds in the forward direction? 3 Sn4+(aq) + 2 Cr(s) → 3 Sn2+(aq) + 2 Cr3+(aq)

Accepted Answer

A)   Sn4+(aq) is the reducing agent and Cr(s) is the oxidizing agent.
B)   Cr(s) is the reducing agent and Sn2+(aq) is the oxidizing agent.
C)   Sn4+(aq) is the reducing agent and Sn2+(aq) is the oxidizing agent.
D)   Cr(s) is the reducing agent and Cr3+(aq) is the oxidizing agent.
E)   Cr(s) is the reducing agent and Sn4+(aq) is the oxidizing agent.F) A) and C)
G) A) and E)

Question 14

Write the balanced reduction half-reaction for the following overall reaction: 2 Fe(s) + 3 Cl2(aq) → 2 Fe3+(aq) + 6 Cl-(aq)

Accepted Answer

A)   Cl2(aq) + 2 e- → 2 Cl-(aq) 
B)   Fe(s) + 3 e- → Fe3+(aq) 
C)   Fe(s) + Cl2(aq) → FeCl3(aq) 
D)   Cl2(aq) → 2 Cl-(aq) + 2 e-
E)   3 Cl2(aq) + 2 e- → 2 Cl-(aq) F) B) and D)
G) A) and D)

Question 15

Write a balanced half-reaction for the reduction of hydrogen peroxide to water in an acidic solution.

Accepted Answer

A)   2 H2O2( 2O2(   ) → 2 H2O(   ) + O2(g)  
B)   2 H2O2(   ) + 2e- → 2 H2O(   ) + O2(g)  
C)   H2O2(   ) + 2 H+(aq) + 2 e- → 2 H2O(   )  
D)   H2O2(   ) + 4 H+(aq) + 2 e- → 2 H2O(   ) + H2(g)  
E)   H2O2(   ) + 2 H+(aq) + 4 e- → 2 H2(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > ) → 2 H2O( 2O2(   ) → 2 H2O(   ) + O2(g)  
B)   2 H2O2(   ) + 2e- → 2 H2O(   ) + O2(g)  
C)   H2O2(   ) + 2 H+(aq) + 2 e- → 2 H2O(   )  
D)   H2O2(   ) + 4 H+(aq) + 2 e- → 2 H2O(   ) + H2(g)  
E)   H2O2(   ) + 2 H+(aq) + 4 e- → 2 H2(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > ) + O2(g) 
B)   2 H2O2( 2O2(   ) → 2 H2O(   ) + O2(g)  
B)   2 H2O2(   ) + 2e- → 2 H2O(   ) + O2(g)  
C)   H2O2(   ) + 2 H+(aq) + 2 e- → 2 H2O(   )  
D)   H2O2(   ) + 4 H+(aq) + 2 e- → 2 H2O(   ) + H2(g)  
E)   H2O2(   ) + 2 H+(aq) + 4 e- → 2 H2(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > ) + 2e- → 2 H2O( 2O2(   ) → 2 H2O(   ) + O2(g)  
B)   2 H2O2(   ) + 2e- → 2 H2O(   ) + O2(g)  
C)   H2O2(   ) + 2 H+(aq) + 2 e- → 2 H2O(   )  
D)   H2O2(   ) + 4 H+(aq) + 2 e- → 2 H2O(   ) + H2(g)  
E)   H2O2(   ) + 2 H+(aq) + 4 e- → 2 H2(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > ) + O2(g) 
C)   H2O2( 2O2(   ) → 2 H2O(   ) + O2(g)  
B)   2 H2O2(   ) + 2e- → 2 H2O(   ) + O2(g)  
C)   H2O2(   ) + 2 H+(aq) + 2 e- → 2 H2O(   )  
D)   H2O2(   ) + 4 H+(aq) + 2 e- → 2 H2O(   ) + H2(g)  
E)   H2O2(   ) + 2 H+(aq) + 4 e- → 2 H2(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > ) + 2 H+(aq) + 2 e- → 2 H2O( 2O2(   ) → 2 H2O(   ) + O2(g)  
B)   2 H2O2(   ) + 2e- → 2 H2O(   ) + O2(g)  
C)   H2O2(   ) + 2 H+(aq) + 2 e- → 2 H2O(   )  
D)   H2O2(   ) + 4 H+(aq) + 2 e- → 2 H2O(   ) + H2(g)  
E)   H2O2(   ) + 2 H+(aq) + 4 e- → 2 H2(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > ) 
D)   H2O2( 2O2(   ) → 2 H2O(   ) + O2(g)  
B)   2 H2O2(   ) + 2e- → 2 H2O(   ) + O2(g)  
C)   H2O2(   ) + 2 H+(aq) + 2 e- → 2 H2O(   )  
D)   H2O2(   ) + 4 H+(aq) + 2 e- → 2 H2O(   ) + H2(g)  
E)   H2O2(   ) + 2 H+(aq) + 4 e- → 2 H2(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > ) + 4 H+(aq) + 2 e- → 2 H2O( 2O2(   ) → 2 H2O(   ) + O2(g)  
B)   2 H2O2(   ) + 2e- → 2 H2O(   ) + O2(g)  
C)   H2O2(   ) + 2 H+(aq) + 2 e- → 2 H2O(   )  
D)   H2O2(   ) + 4 H+(aq) + 2 e- → 2 H2O(   ) + H2(g)  
E)   H2O2(   ) + 2 H+(aq) + 4 e- → 2 H2(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > ) + H2(g) 
E)   H2O2( 2O2(   ) → 2 H2O(   ) + O2(g)  
B)   2 H2O2(   ) + 2e- → 2 H2O(   ) + O2(g)  
C)   H2O2(   ) + 2 H+(aq) + 2 e- → 2 H2O(   )  
D)   H2O2(   ) + 4 H+(aq) + 2 e- → 2 H2O(   ) + H2(g)  
E)   H2O2(   ) + 2 H+(aq) + 4 e- → 2 H2(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > ) + 2 H+(aq) + 4 e- → 2 H2(g) + O2(g) F) All of the above
G) A) and B)

Question 16

The following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H2(g,1.00 atm) | H+(aq,1.00 M) || Cl-(aq) | AgCl(s) | Ag
The standard reduction potential,E°,of AgCl(s) is +0.222 V.Calculate the Cl-(aq) ion concentration.

Accepted Answer

A)   1.9 × 10-19 M
B)   5.5 × 10-10 M
C)   0.018 M
D)   1.03 M
E)   1.8 × 109 MF) A) and B)
G) B) and E)

Question 17

For the electrochemical cell Cu(s) | Cu2+ || Ag+ | Ag(s) ,the standard cell potential is 0.46 V.A cell using these reagents was made,and the observed potential was 0.26 V at 25 oC.Which of the following is a possible explanation for the observed voltage?

Accepted Answer

A)   The volume of the Cu2+ solution was larger than the volume of the Ag+ solution.
B)   The volume of the Ag+ solution was larger than the volume of the Cu2+ solution.
C)   The Cu2+ concentration was larger than the Ag+ concentration.
D)   The Ag electrode was twice as large as the Cu electrode.
E)   The Ag+ concentration was larger than the Cu2+ concentration.F) None of the above
G) C) and D)

Question 18

Aluminum(III) ion (Al3+) is reduced to solid aluminum at an electrode.If a current of 2.75 amperes is passed for 36 hours,calculate the mass of aluminum deposited at the electrode.(Assume 100% current efficiency.)

Accepted Answer

A)   9.2 × 10-3 g
B)   3.3 × 101 g
C)   9.9 × 101 g
D)   1.0 × 102 g
E)   3.0 × 102 gF) B) and D)
G) A) and B)

Question 19

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu2+(aq) + Fe(s) → Cu(s) + Fe2+(aq)

Accepted Answer

A)   Cu(s) | Cu2+(aq) || Fe2+(aq) | Fe(s) 
B)   Fe(s) || Fe2+(aq) ,Cu2+(aq) | Cu(s) 
C)   Cu(s) || Cu2+(aq) ,Fe2+(aq) || Fe(s) 
D)   Cu(s) | Fe2+(aq) || Cu2+(aq) | Fe(s) 
E)   Fe(s) | Fe2+(aq) || Cu2+(aq) | Cu(s) F) D) and E)
G) A) and D)

Question 20

An SHE electrode has been assigned a standard reduction potential,E°,of 0.00 volts.Which of the following reactions will occur at this electrode?

Accepted Answer

A)   2 H2O( 2O(   ) + 2 e- → H2(g) + 2 OH-(aq)  
B)   O2(g) + 4 e- → 2 O2-(aq)  
C)   Hg2Cl2(s) + 2 e- → 2 Hg(   ) + 2 Cl-(aq)  
D)   Li+(aq) + e- → Li(s)  
E)   2 H+(aq) + 2 e- → H2(g) " class="answers-bank-image d-inline" rel="preload" > ) + 2 e- → H2(g) + 2 OH-(aq) 
B)   O2(g) + 4 e- → 2 O2-(aq) 
C)   Hg2Cl2(s) + 2 e- → 2 Hg( 2O(   ) + 2 e- → H2(g) + 2 OH-(aq)  
B)   O2(g) + 4 e- → 2 O2-(aq)  
C)   Hg2Cl2(s) + 2 e- → 2 Hg(   ) + 2 Cl-(aq)  
D)   Li+(aq) + e- → Li(s)  
E)   2 H+(aq) + 2 e- → H2(g) " class="answers-bank-image d-inline" rel="preload" > ) + 2 Cl-(aq) 
D)   Li+(aq) + e- → Li(s) 
E)   2 H+(aq) + 2 e- → H2(g) F) A) and D)
G) C) and D)

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Which of the following statements is true for the following reaction,assuming the given reaction proceeds in the forward direction? 3 Sn⁴⁺(aq) + 2 Cr(s) → 3 Sn²⁺(aq) + 2 Cr³⁺(aq)

Correct Answer
verified

Which of the following reactions will require the use of an inert electrode when used in a voltaic cell?

Correct Answer
verified

When the given oxidation-reduction reaction in an acidic solution is balanced,what is the lowest whole-number coefficient for H⁺,and on which side of the balanced equation should it appear? MnO₄^-(aq) + Br^-(aq) → Mn²⁺(aq) + Br₂(l)

Correct Answer
verified

Aluminum(III) ion (Al³⁺) is reduced to solid aluminum at an electrode.If a current of 2.75 amperes is passed for 36 hours,calculate the mass of aluminum deposited at the electrode.(Assume 100% current efficiency.)

Correct Answer
verified

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Fe(s) → Cu(s) + Fe²⁺(aq)

Correct Answer
verified

Correct Answer
verified

Which of the following overall chemical equations is responsible for generating electricity in fuel cells used in NASA's Space Shuttle programs?

Correct Answer
verified

An SHE electrode has been assigned a standard reduction potential,E°,of 0.00 volts.Which of the following reactions will occur at this electrode?

Correct Answer
verified

Write a balanced half-reaction for the reduction of hydrogen peroxide to water in an acidic solution.

Correct Answer
verified

In the context of the diagram given below,which of the following statements is true concerning half-cell II?

Correct Answer
verified

The following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H₂(g,1.00 atm) | H⁺(aq,1.00 M) || Cl^-(aq) | AgCl(s) | Ag The standard reduction potential,E°,of AgCl(s) is +0.222 V.Calculate the Cl^-(aq) ion concentration.

Correct Answer
verified

The following has a potential of 0.34 V. If the concentrations of each of the ions is 1.0 M and the pressure of H₂ is 1.0 atm,then E° for the half-reaction is _____.

Correct Answer
verified

Which of the following statements concerning voltaic cells is not true?

Correct Answer
verified

Primary batteries are also called storage batteries or rechargeable batteries.

Correct Answer
verified

Calculate the standard cell potential ( ) for the reaction 2 Ag(s) + Co²⁺(aq) → 2 Ag⁺(aq) + Co(s) . The standard reduction potentials are as follows: Ag⁺(aq) + e⁻→ Ag(s) E° = 0.8 V Co²⁺(aq) +2 e⁻→ Co(s) E° = -0.277 V

Correct Answer
verified

For the following cell reaction,the standard cell potential is 1.34 V.To determine the cell potential at nonstandard conditions,what is the value that should be used for n in the Nernst equation?

Correct Answer
verified

Correct Answer
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For the electrochemical cell Cu(s) | Cu²⁺ || Ag⁺ | Ag(s) ,the standard cell potential is 0.46 V.A cell using these reagents was made,and the observed potential was 0.26 V at 25 ^oC.Which of the following is a possible explanation for the observed voltage?

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Write a balanced half-reaction for the reduction of CrO₄^2-(aq) to Cr(OH) ₃(s) in a basic solution.

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Write the balanced reduction half-reaction for the following overall reaction: 2 Fe(s) + 3 Cl2(aq) → 2 Fe3+(aq) + 6 Cl-(aq)

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Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Which of the following statements is true for the following reaction,assuming the given reaction proceeds in the forward direction? 3 Sn4+(aq) + 2 Cr(s) → 3 Sn2+(aq) + 2 Cr3+(aq)

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Which of the following reactions will require the use of an inert electrode when used in a voltaic cell?

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When the given oxidation-reduction reaction in an acidic solution is balanced,what is the lowest whole-number coefficient for H+,and on which side of the balanced equation should it appear? MnO4-(aq) + Br-(aq) → Mn2+(aq) + Br2(l)

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Aluminum(III) ion (Al3+) is reduced to solid aluminum at an electrode.If a current of 2.75 amperes is passed for 36 hours,calculate the mass of aluminum deposited at the electrode.(Assume 100% current efficiency.)

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Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu2+(aq) + Fe(s) → Cu(s) + Fe2+(aq)

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Calculate Ecell for the following electrochemical cell at 25 °C Pt(s) | H2(g,1.00 atm) | H+(aq,1.00 M) || Sn2+(aq,0.350 M) ,Sn4+(aq,0.020 M) | Pt(s) The standard reduction potentials are as follows: Sn4+(aq) + 2 e- → Sn2+(s) E° = +0.15 V 2 H+(aq) + 2 e- → H2(g) E° = 0.00 V

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Which of the following overall chemical equations is responsible for generating electricity in fuel cells used in NASA's Space Shuttle programs?

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An SHE electrode has been assigned a standard reduction potential,E°,of 0.00 volts.Which of the following reactions will occur at this electrode?

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Write a balanced half-reaction for the reduction of hydrogen peroxide to water in an acidic solution.

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In the context of the diagram given below,which of the following statements is true concerning half-cell II?

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The following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H2(g,1.00 atm) | H+(aq,1.00 M) || Cl-(aq) | AgCl(s) | Ag The standard reduction potential,E°,of AgCl(s) is +0.222 V.Calculate the Cl-(aq) ion concentration.

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The following has a potential of 0.34 V. If the concentrations of each of the ions is 1.0 M and the pressure of H2 is 1.0 atm,then E° for the half-reaction is _____.

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Which of the following statements concerning voltaic cells is not true?

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Primary batteries are also called storage batteries or rechargeable batteries.

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Calculate the standard cell potential ( ) for the reaction 2 Ag(s) + Co2+(aq) → 2 Ag+(aq) + Co(s) . The standard reduction potentials are as follows: Ag+(aq) + e−→ Ag(s) E° = 0.8 V Co2+(aq) +2 e−→ Co(s) E° = -0.277 V

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For the following cell reaction,the standard cell potential is 1.34 V.To determine the cell potential at nonstandard conditions,what is the value that should be used for n in the Nernst equation?

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Calculate the equilibrium constant for the following reaction at 25 °C, 2 IO3-(aq) + 5 Hg( ) + 12 H+(aq) → I2(s) + 5 Hg2+(aq) + 6 H2O( ) The standard reduction potentials are as follows: IO3-(aq) + 6 H+(aq) + 5 e- → I2(s) + 3 H2O( ) E° = +1.20 V Hg2+(aq) + 2 e- → Hg( ) E° = +0.86 V

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For the electrochemical cell Cu(s) | Cu2+ || Ag+ | Ag(s) ,the standard cell potential is 0.46 V.A cell using these reagents was made,and the observed potential was 0.26 V at 25 oC.Which of the following is a possible explanation for the observed voltage?

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Write a balanced half-reaction for the reduction of CrO42-(aq) to Cr(OH) 3(s) in a basic solution.

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Write the balanced reduction half-reaction for the following overall reaction: 2 Fe(s) + 3 Cl2(aq) → 2 Fe3+(aq) + 6 Cl-(aq)

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Which of the following statements is true for the following reaction,assuming the given reaction proceeds in the forward direction? 3 Sn⁴⁺(aq) + 2 Cr(s) → 3 Sn²⁺(aq) + 2 Cr³⁺(aq)

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When the given oxidation-reduction reaction in an acidic solution is balanced,what is the lowest whole-number coefficient for H⁺,and on which side of the balanced equation should it appear? MnO₄^-(aq) + Br^-(aq) → Mn²⁺(aq) + Br₂(l)

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Aluminum(III) ion (Al³⁺) is reduced to solid aluminum at an electrode.If a current of 2.75 amperes is passed for 36 hours,calculate the mass of aluminum deposited at the electrode.(Assume 100% current efficiency.)

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Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Fe(s) → Cu(s) + Fe²⁺(aq)

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The following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H₂(g,1.00 atm) | H⁺(aq,1.00 M) || Cl^-(aq) | AgCl(s) | Ag The standard reduction potential,E°,of AgCl(s) is +0.222 V.Calculate the Cl^-(aq) ion concentration.

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The following has a potential of 0.34 V. If the concentrations of each of the ions is 1.0 M and the pressure of H₂ is 1.0 atm,then E° for the half-reaction is _____.

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Calculate the standard cell potential ( ) for the reaction 2 Ag(s) + Co²⁺(aq) → 2 Ag⁺(aq) + Co(s) . The standard reduction potentials are as follows: Ag⁺(aq) + e⁻→ Ag(s) E° = 0.8 V Co²⁺(aq) +2 e⁻→ Co(s) E° = -0.277 V

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For the electrochemical cell Cu(s) | Cu²⁺ || Ag⁺ | Ag(s) ,the standard cell potential is 0.46 V.A cell using these reagents was made,and the observed potential was 0.26 V at 25 ^oC.Which of the following is a possible explanation for the observed voltage?

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Write a balanced half-reaction for the reduction of CrO₄^2-(aq) to Cr(OH) ₃(s) in a basic solution.

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