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F=96485 C mol -1 ,    R=8.314 J mol -1 K -1 ,      T=298 K Part A U...

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F=96485 C mol-1,    R=8.314 J mol-1 K-1,      T=298 K

Part A

Using the table below, calculate the equilibrium constant for the electrochemical cell represented by the following line notation:

Cr(s)|Cr3+(aq)||Fe2+(aq)|Fe(s)

Express your answer to two significant figures.

K 

=

Part B

For the reaction above, calculate the standard Gibbs energy change.

Write your answer to three significant figures.

ΔrG° =

kJ/mol

Part C

Based on your answer in Part B, identify the spontaneity of the reaction:

The above redox reaction is

Standard Electrode Potentials at 25ºC      Eº(V)

Ag+(aq)+e−

→Ag(s)

0.80

Pb2+(aq)+2e−

→Pb(s)

-0.13

Ni2+(aq)+2e−

→Ni(s)

-0.23

Co2+(aq)+2e−

→Co(s)

-0.28

Cd2+(aq)+2e−

→Cd(s)

-0.40

Fe2+(aq)+2e−

→Fe(s)

-0.45

Cr3+(aq)+3e−

→Cr(s)

-0.73

Zn2+(aq)+2e−

→Zn(s)

-0.76

Mn2+(aq)+2e−

→Mn(s)

-1.18

Al3+(aq)+3e−

→Al(s)

-1.66

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