Asked by EBB
What is the equilibrium constant for the redox reaction in question 3?
Combining the two equations for ∆Go below ∆G= −n F Ecell and ∆G= −R T ln K
gives −n F E cell = −R T ln K...
The ecell from question three was .73V
The delta g from question three = −(6 mol) (96, 485C/mol)(0.73 V) = −423 kJ
Is R in this equation 8.314 J/mol * K? And T wasn't specified, so I'm assuming it was 298 K. If these are the correct numbers, why doesn't moles from the constant R cancel? The correct answer is 2.8 × 10^30, but I cannot arrive at that answer. Please let me know if you need clarification.
Combining the two equations for ∆Go below ∆G= −n F Ecell and ∆G= −R T ln K
gives −n F E cell = −R T ln K...
The ecell from question three was .73V
The delta g from question three = −(6 mol) (96, 485C/mol)(0.73 V) = −423 kJ
Is R in this equation 8.314 J/mol * K? And T wasn't specified, so I'm assuming it was 298 K. If these are the correct numbers, why doesn't moles from the constant R cancel? The correct answer is 2.8 × 10^30, but I cannot arrive at that answer. Please let me know if you need clarification.
Answers
There are no human answers yet.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.