2. Consider the following unbalanced redox reaction which is being used to run a

Question

2. Consider the following unbalanced redox reaction which is being used to run a voltaic cell AL, + Cd2.ag) Al,"u, tca, 1(educed a. Write the balanced oxidation half-reaction for this cel b. Write the balanced reduction half-reaction for this cell. -40 voHs Write a balanced chemical equation that describes the overall cell reaction. c. 2 A11 30811 d. Assuming that the cell is operating at standard conditions, what would be the potential of the cell in volts? (1,66 valt) t(40 volh) 1.26 volks = 0.00010 M, what would be the potential of If [AP+] = 2.0 M and [Cd the cell in volts at 25°C? e. I 0

Explanation / Answer

The calculations and equations all are correct.

E. Use Nernst equation,

E = Eo - 0.0592/n logK

K = ([Al3+]^2/[Cd2+]^3)

with,

Eo = 1.26 V

n = 6

we get,

E = 1.26 - 0.0592/6 log[(2)^2/(0.0001)^3]

   = 1.136 V

So, the potential of the cell at 25 oC is 1.136V

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