Asked by Nora
Provide the balanced reaction, the value of K, and E(cell) at equilibrium for the for the electrochemical cell created
from the two half-cell reactions below
Cr^(3+) + e ==> Cr^(2+)
Fe^(2+) + 2e ==> Fe
Well, I got the balanced reaction:
2Cr^(2+) + Fe^(2+) ==> Fe + 2Cr^(3+)
And the E(cell) = 0.06 V.
However, I have no idea how you could possibly solve for K. There doesn't seem to be enough information available to do that.
Help?
from the two half-cell reactions below
Cr^(3+) + e ==> Cr^(2+)
Fe^(2+) + 2e ==> Fe
Well, I got the balanced reaction:
2Cr^(2+) + Fe^(2+) ==> Fe + 2Cr^(3+)
And the E(cell) = 0.06 V.
However, I have no idea how you could possibly solve for K. There doesn't seem to be enough information available to do that.
Help?
Answers
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