Question

# A standard state galvanic cell is constructed from the half-cells described below. Half-Cell 1: Copper rod...

A standard state galvanic cell is constructed from the half-cells described below.

Half-Cell 1: Copper rod in a solution containing 1.00 M Cu(NO3)2

Half-Cell 2: Silver rod in a solution containing 1.00 M AgNO3

a. Draw a diagram of the cell. Label the anode and cathode. Indicate the direction of electron flow

across the wire and ion flow through the salt bridge.

Write a balanced chemical equation for the cell reaction and calculate the E‹ and ΔG‹ for it.

E‹:____________________________

ΔG‹:____________________________

c. The cell is allowed to run until the reaction reaches equilibrium. Calculate the concentration of

each ion at this point.

Q1

anode is the one in which oxidation occurs (left side)

cathode --> righ side, Ag will reduce

flow goes from left to right

For

E°cell

Cu2+ + 2 e− ⇌ Cu(s) +0.337

Ag+ + e− ⇌ Ag(s) +0.7996

Copper has lower potential, so it will oxidize first

E°cell = 0.7996 - 0.337 = 0.7996 V

for

dG

dG = -nF*E°cell

dG = -2*96500*0.7996

dG = -154322.8 J/mol = -154.32 kJ/mol

c)

calcualte concnetration of each ion at this point...

assume

Ecell is 99% gones so

[Ag+] = 0.01 M

[Cu+2] = 1.99 M