We're being asked to determine the change in the mass of the anode.
It is mentioned that the cell is a voltaic cell. For this to be a voltaic cell:
• ↓ E° → oxidation → anode
Loss Electrons → Oxidation
• ↑ E° → reduction → cathode
Gain Electrons → Reduction
Cu(NO3)2 and AgNO3 are both ionic compounds and will break up in the solution:
Cu(NO3)2(aq) → Cu2+(aq) + 2 NO3‒(aq)
AgNO3(aq) →Ag+(aq) + NO3‒(aq)
Refer to the standard reduction potential table:
You construct of voltaic cell with standard concentrations of solutions using Cu(NO 3)2 and a Cu electrode as well as AgNO3 and a Ag electrode. After the cell has been operating for some time you find that the mass of the cathode has increased by 1 g. How much has the mass of the anode changed?
A. it is 0.29 g less.
B. it is 0.29 g more.
C. it is 1 g less.
D. it is 0.58 g more.
E. it is 3.39 g less.
F. the anode mass is unchanged
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