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11 Dec 2019

balance the following redox reaction in basic solution Ag(s)+CN-(aq)+ O2(g) -->Ag (CN)2- (aq)

cyanide is not participating in the electrochemical reaction but does associate with the silver ion formed in a second association reaction. Balance the electrochemistry first and then add in the cyanide in by adding an associative reaction to the redox reaction.

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Collen Von
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13 Dec 2019

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Related questions

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.

Gold exists in two common positive oxidation states, +1 and +3. The standard reduction potentials for these oxidation states are

Au+(aq) + e– Au(s) E°red = +1.69 V

Au3+(aq) + 3 e– Au(s) E°red = +1.50 V

(a) Can you use these data to explain why gold does not tarnish in the air? (b) Suggest several substances that should be strong enough oxidizing agents to oxidize gold metal. (c) Miners obtain gold by soaking gold-containing ores in an aqueous solution of sodium cyanide. A very soluble complex ion of gold forms in the aqueous solution because of the redox reaction

4 Au(s) + 8 NaCN(aq) + 2 H2O(l) + O2(g) 4 Na[Au(CN)2](aq) + 4 NaOH(aq)

What is being oxidized and what is being reduced in this reaction? (d) Gold miners then react the basic aqueous product solution from part (c) with Zn dust to get gold metal. Write a balanced redox reaction for this process. What is being oxidized, and what is being reduced?

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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