Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2C12*(aq) + H2(g)2Cu*(aq) + 2H'(aq) Answer: kJ K for this reaction would be than one. Ret greater less Submit Answer 9 more group attempts remaining

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2C12(aq) + H2(g)2Cu(aq) + 2H'(aq) Answer: kJ K for this reaction would be than one. Ret greater less Submit Answer 9 more group attempts remaining

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter21: Transition Metals And Coordination Chemistry

Section: Chapter Questions

Problem 77AE

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Question

Part.a

Part.b

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction:
2CU2*(aq) + H2(g)2Cu*(aq) + 2H'(aq)
Answer:
kJ
K for this reaction would be
than one.
Ret greater
less
Submit Answer
9 more group attempts remaining

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction:
2Cu2"(aq) + Cu(s)2Cu*(aq) + Cu²*(aq)
Answer:
kJ
K for this reaction wopld be
than one.
Submit Answer
Retry Entire Group
9 more group attempts remaining

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An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Consider the following galvanic cell: Label the reducing agent and the oxidizing agent, and describe the direction of the electron flow.
The equation G = nF also can be applied to half-reactions. Use standard reduction potentials to estimate Gf for Fe2+ (aq) and Fe3+ (aq). Gf for e= 0.)
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The overall reaction for the production of Cu(OH)2 from Cu in oxygenated water can be broken into three steps: an oxidation half-reaction, a reduction half-reaction, and a precipitation reaction. a. Complete and balance the two missing half-reactions to give the overall equation for the oxidation of cooper in seawater. Oxidation half-reaction: ? Reduction half-reaction: ? Precipitation:Cu2+(aq)+2OH(aq)Cu(OH)2(s)Overall:Cu(s)+12O2(g)+H2O(l)Cu(OH)2(s) b. Determine the equilibrium constant for the overall reaction at 25 C using standard reduction potentials and the solubility product constant (Ksp) of Cu(OH)2(s).
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One of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce1,4-dicyanobutane. The reduction reaction is 2CH2CHCH+2H++2eNC(CH2)4CN The NC(CH2)4CN is then chemically reduced using hydrogen gas to H2N(CH2)6NH2, which is used in the production of nylon. What current must be used to produce 150.kg NC(CH2)4CN per hour?
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