Solution Found!
An electrochemical cell is set up with 1 M Pb(NO3)2 on one side, and 1 M AgNO3 on the
Chapter 0, Problem 5(choose chapter or problem)
An electrochemical cell is set up with \(1\mathrm{\ M}\mathrm{\ Pb}\left(\mathrm{NO}_3\right)_2\) on one side, and \(1\mathrm{\ M\ }\mathrm{AgNO}_3\) on the other.
a. Which metal will be oxidized? Which will be reduced? Write out balanced half-reactions for these reactions.
b. Write out the balanced overall reaction for this electrochemical cell.
c. How many moles of electrons will flow from the anode to the cathode?
d. Calculate the voltage for this electrochemical cell.
Questions & Answers
QUESTION:
An electrochemical cell is set up with \(1\mathrm{\ M}\mathrm{\ Pb}\left(\mathrm{NO}_3\right)_2\) on one side, and \(1\mathrm{\ M\ }\mathrm{AgNO}_3\) on the other.
a. Which metal will be oxidized? Which will be reduced? Write out balanced half-reactions for these reactions.
b. Write out the balanced overall reaction for this electrochemical cell.
c. How many moles of electrons will flow from the anode to the cathode?
d. Calculate the voltage for this electrochemical cell.
ANSWER:Step 1 of 5
It is possible to determine the anode and the cathode based on the reduction potential values.
The anode is where oxidation occurs and has a low standard reduction potential value.
The cathode is where reduction occurs and has a high standard reduction potential value.