You make a galvanic cell with chromium metal in 0.10 M Cr(NO3)3 solution as one half-cell (Eo = -0.74 V) and silver metal in 0.10 M Ag(NO3) solution at the other half-cell (Eo = + 0.80 V). 1. Which half-cell undergoes reduction? 2. What is the half-reaction that describes the chemistry at the anode? 3. What is the balanced net ionic equation for the overall reaction of the cell?
For all of the questions, consider the following:
You make a galvanic cell with chromium metal in 0.10 M Cr(NO3)3 solution as one half-cell (Eo = -0.74 V) and silver metal in 0.10 M Ag(NO3) solution at the other half-cell (Eo = + 0.80 V).
4. What is the standard cell potential for the galvanic cell? Calculate this in volts, and enter just the numerical value (aka, no need to include the unit V).
5. If you ran the cell as you made it above, what would it's cell potential be? The cell is still at atmospheric pressure and standard temperature. The cell was made with chromium metal in 0.10 M Cr(NO3)3 solution and silver metal in 0.10 M Ag(NO3) solution. Calculate this in volts, and enter just the numerical value (aka, no need to include the unit V).
A silver chromium voltaic cell is a type of electrochemical cell that generates an electric current through an oxidation-reduction reaction. It consists of two electrodes, one made of silver (Ag) and the other of chromium (Cr), immersed in an electrolyte solution. The silver electrode serves as the anode and the chromium electrode serves as the cathode.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
