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10 Nov 2019

1. A) Calculate the EoCell and the Gibbs free energy for the following cell diagram

Ni(s)|Ni2+(aq)||Ag+(aq)|Ag(s)

B) Balance the following redox reaction H2S(aq) + Cl2(g) -----> S(s) + Cl-(aq)

C) Determine the unknown concentration of the ion in the following cell: Pb(s)|Pb2+(aq, ?)||Ni2+(aq, 0.20 M|Ni(s), E = +0.050 V.

D) How much time is required to electroplate 1.50 g of silver from a silver nitrate solution by using a current of 13.6 mA.

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30 Oct 2019

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Related questions

Which electrochemical reaction is spontaneous in a galvanic cell?

Ni2+(aq) + Cu(s) --> Ni(s) + Cu2+(aq)

Cr3+(aq) + Au(s) --> Cr(s) + Au3+(aq)

Cu2+(aq) + Co2+(aq) --> Cu+(aq) + Co3+(aq)

Cu2+(aq) + Sn(s) --> Cu(s) + Sn2+(aq)

Which electrochemical reaction is non-spontaneous in an electrolytic cell?

F2(g) + 2Cl-(aq) --> 2F-(aq) + Cl2(g)

Ag+(aq) + Fe2+(aq) --> Ag(s) + Fe3+(aq)

Co2+(aq) + Pb(s) --> Co(s) + Pb2+(aq)

Mn2+(aq) + Ba(s) --> Mn(s) + Ba2+(aq)

Which electrochemical reaction is the most spontaneous, generating the highest cell voltage?

F2(g) + 2Cl-(aq) --> 2F-(aq) + Cl2(g)

Ag+(aq) + Fe2+(aq) --> Ag(s) + Fe3+(aq)

Mn2+(aq) + Ba(s) --> Mn(s) + Ba2+(aq)

Cu2+(aq) + Sn(s) --> Cu(s) + Sn2+(aq)

Given the following notation for a galvanic cell diagram

Cd(s) │ Cd2+(aq) ║ Pb2+(aq) │ Pb(s)

Which one correctly represents the electrochemical reaction taking place in the galvanic cell?

Cd(s) + Pb2+(aq) --> Cd2+(aq) + Pb(s)

Cd2+(aq)+ Pb2+(aq) --> Cd(s)+ Pb(s)

Cd2+(aq) + Pb(s) --> Cd(s) + Pb2+(aq)

Cd2+(aq) + Pb2+(aq) --> Cd(s) + Pb2+(s)

Consider a Galvanic cell constructed from the following half cells, linked by a KCl salt bridge.

. an Al(s) electrode in 0.5 M Al2(SO4)3 solution

. a Pb(s) electrode in 1.0 M Pb(NO3)2 solution

Which electrode is the cathode?

Al

Pb

Al3+

Pb2+

What is the standard emf of a galvanic cell made of a Co electrode in a 1.0 M Co(NO3)2 solution and a Al electrode in a 1.0 M Al(NO3)3 solution at 25°C?

A. A voltaic cell is constructed based on the reaction of Ag(CN)2-(aq) with Cr(s) producing Ag(s) and Cr3+(s). Identify the correct cell diagram.

a.

Ag(CN)2-(aq) | Cr(s) || Ag(s) | Cr3+(aq)

d.

Ag(CN)2-(aq) | Ag(s) || Cr(s) | Cr3+(aq)

b.

Ag(s) | Cr3+(aq) || Ag(CN)2-(aq) | Cr(s)

e.

Cr(s) | Cr3+(aq) || Ag(CN)2-(aq) | Ag(s)

c.

Cr(s) | Cr3+(aq) || Ag(s) | Ag(CN)2-(aq)

B. Use the table of standard reduction potentials below to identify the metal or metal ion that is the strongest oxidizing agent.

Half-reaction

Pb4+ + 2 e- ® Pb2+

+1.80

Au3+ + 3 e- ® Au

+1.50

Fe3+ + 3 e- ® Fe

+0.771

I2 + 2 e- ® 2 I-

+0.535

Pb2+ + 2 e- ® Pb

-0.124

Al3+ + 3 e- ® Al

-1.66

Mg2+ + 2 e- ® Mg

-2.37

K+ + e- ® K

-2.93

a.

Pb4+

d.

K

b.

Pb2+

e.

Al

c.

K+

C. Silver tarnish (Ag2S) can be removed by immersing silverware in a hot solution of baking soda (NaHCO3) in a pan lined with aluminum foil; however, foul-smelling hydrogen sulfide gas (H2S) is produced. Which of the following statements is correct?

Silver/silver(I)

+0.799

Sulfur/hydrogen sulfide

+0.141

Aluminum/aluminum(III)

-1.662

Sodium/sodium(I)

-2.713

a.

Aluminum ions react with S2-, form aluminum sulfide, and gaseous carbon dioxide is released.

b.

Silver ions in the presence of the baking soda (NaHCO3) oxidize sulfide to elemental sulfur that attacks the aluminum foil, which produces aluminum sulfide.

c.

The aluminum acts as a reducing agent for the silver(I) in silver sulfide; then bicarbonate ion protonates the sulfide ion that is released.

d.

Aluminum is plated onto the silver surface, making it shiny again, and then the reaction of bicarbonate with aluminum oxide releases CO2.

e.

Silver in Ag2S reduces the aluminum, becomes metallic silver in the process, and releases hydrogen sulfide, H2S.

D. Using the following data, determine the standard cell potential for the electrochemical cell constructed using the following reaction: Zn(s) + Pb2+(aq) ® Zn2+(aq) + Pb(s).

Half-reaction Standard reduction potential

Zn2+(aq) + 2 e- ® Zn(s) -0.763

Pb2+(aq) + 2 e- ® Pb(s) -0.126

a.

+0.637 V

d.

-0.889 V

b.

-0.637 V

e.

+0.889 V

c.

+1.274 V

E. Based on the information in the table of standard reduction potentials below, what is the standard cell potential for an electrochemical cell that has iron (Fe) and magnesium (Mg) electrodes immersed in 1M Fe3+ and Mg2+ solutions? Also, identify the cathode.

Half-reaction

Pb4+ + 2 e- ® Pb2+

+1.80

Au3+ + 3 e- ® Au

+1.50

Fe3+ + 3 e- ® Fe

+0.771

I2 + 2 e- ® 2 I-

+0.535

Pb2+ + 2 e- ® Pb

-0.124

Al3+ + 3 e- ® Al

-1.66

Mg2+ + 2 e- ® Mg

-2.37

K+ + e- ® K

-2.93

a.

+1.60 V with Fe as the cathode

d.

-3.14 V with Mg as the cathode

b.

+3.14 V with Mg as the cathode

e.

+3.14 V with Fe as the cathode

c.

-3.14 V with Fe as the cathode


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