Recent content by kumarium

Thank you for the help!

The equation that should be most likely used is E = E°-(0.0592/n)(logk). 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 =...

E°cell = E°cathode - E°anode E°cell = (RT/nF)(lnk) E = E° - (0.0592/n)(logk)

What is the equation I should be using for the following question: 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!