- #1

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At 298K a cell reaction has a standard emf of +0.17V. The equilibrium constant for the cell reaction is 5.5 X 10^5. What is the value of n for the cell reaction.

Grateful for anyone's help!

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- Thread starter kumarium
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- #1

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At 298K a cell reaction has a standard emf of +0.17V. The equilibrium constant for the cell reaction is 5.5 X 10^5. What is the value of n for the cell reaction.

Grateful for anyone's help!

- #2

Borek

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What equations have you learned while studying redox potentials?

- #3

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E°cell = E°cathode - E°anode

E°cell = (RT/nF)(lnk)

E = E° - (0.0592/n)(logk)

E°cell = (RT/nF)(lnk)

E = E° - (0.0592/n)(logk)

- #4

Borek

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- #5

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I have the value for the standard emf = E°, and value of k.

Do I assume E to be zero then? If I do so, then the solution should look like the following:

0= E° - (0.0592/n)(logk)

0= 0.17 - (0.0592/n)(log(5.5*10^5))

0.17 = (0.0592/n)(log(5.5*10^5))

n= (0.0592)(log(5.5*10^5)) / 0.17

n= 1.9989

- #6

Borek

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Yes.

When Q=K cell potential is zero.

When Q=K cell potential is zero.

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Thank you for the help!

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