If the equilibrium constant for a two-electron redox reaction at 298 K is 1.8×10
ID: 993522 • Letter: I
Question
If the equilibrium constant for a two-electron redox reaction at 298 K is 1.8×104, calculate the corresponding G and Ecel under standard conditions. (G naught and E naught)
This problem has me confused. It seems to have no quantity of "stuff" that I can plug in. Am I just missing something? If you could walk me through the regular steps of finding G and E and where the "stuff" is in the equation, that would be incredibly helpful.
This is all my chemistry professor gave me so if the problem is to incomplete to perform the proper calculations please let me know too! Thank you!
Explanation / Answer
delta Go = -RT lnK
= - 8.314 J/mol K x 298 K x ln 1.8 x 10-4
= 21.363 kJ
Check for significant figure according to ur proffessor problem.
we knoe
delta Go= - nFE
given n=2 (two electron)
delta Go = -2 x 96500 x E
21.363 x1000 J = -2 x 96500 x E
E= -0.11 V
PROBLEM SOLVED