I included the information below but I just need the answer to Part B. The follo

Question

I included the information below but I just need the answer to Part B.

The following values may be useful when solving this tutorial.

Part A

In the activity, click on the Ecell and Keq quantities to observe how they are related. Use this relation to calculate Keq for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occur in the cell are

Cu2+(aq)+2eCu(s) and Co(s)Co2+(aq)+2e

The net reaction is

Cu2+(aq)+Co(s)Cu(s)+Co2+(aq)

Use the given standard reduction potentials in your calculation as appropriate.

Express your answer numerically to three significant figures.

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Incorrect; correct answer displayed

The use of logarithms in this calculation magnifies differences in the value of Keq due to small rounding differences of the constants used. The displayed accepted answer is that obtained using natural logarithms and the values of the constants R, F, and T listed in the table.

Part B

In the activity, click on the Keq and G quantities to observe how they are related. Calculate G using this relationship and the equilibrium constant (Keq) obtained in Part A at T=298K:

Keq=5.88×1020

Express the Gibbs free energy (G) in joules to three significant figures.

Explanation / Answer

We know that

Delta G = -RTlnKeq

R = gas constant = 8.314

T= temperature = 298 K

Keq = 5.88 X 10^20

G = -8.314 X 298 X ln 5.88 X 10^20 = 2.303 X 8.314 X 298 X log 5.88 X 10^20 = -118.510 KJ / mole

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