Consider the galvanic cell based on the following half-reactions:

Au^3+(aq) + 3 e^-→ Au (s) E° = 1.50 V

Tl^+(aq) + e^-→ Tl (s) E° = -0.34 V

a) Determine the overall cell reaction and calculate E°cell

b) Calculate delta G° and the equilibrium constant K for the cell reaction at 25°C

c) Calculate Ecell at 25°C when [Au3+] = 1.0 x 10^-2M and [Tl+] = 1.0 x 10^-4M. Will the cell potential increase or decrease by increasing the concentration of Au3+?

Expert Answers

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For parts A & B, see

Please note that when you post a question, it should only include *one* question. Dividing it into parts A-C does not make it one question :)

For part C, we need to calculate Ecell under non-standard conditions

Ecell = Eocell - 0.0592/n log Q

We know Eocell and have 1.84V (see link above). To find Q, we have to first write the balanced equation

Au3+(aq) + 3Tl(s) --> Au(s) + 3Tl+(aq)

We need the 3s in front of Tl and Tl+ so that the number of electrons in each reaction is the same so that they will cancel out.  Now, we can find Q

Q = [Tl+]^3 / [Au3+]

Q = (1x10^-4)^3 / 1x10^-2

Q = 1 x 10^-10

Now we can solve for Ecell

Ecell = 1.84 - (0.0592/3) log (1 x 10^-10)

Ecell = 2.04 V

If we increase the concentration of Au3+, then the value of Q will decrease and the log of the value will also decrease.  As a result, the second term will have a greater magnitude so the Ecell will increase because we are substracting a negative term.

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