Question

Cell: Fe(s)| Fe2+(aq, 1M) | Cu2+(aq, 1M) | Cu(S)

Calculated Values

ΔG° = -nFE° = ΔH° - TΔS° ΔH° = -0.34905 J/C * 2 mols * 96485 C/mol = -67,356.18 J =67.36kJ

ΔS° = 0.8597 x 10-3 J/C * 2 mols * 96485 C/mol = 165.89 J

ΔG° =-67356.18 J – (298*165.9 J) = -116794.4 J = -116.79 kJ

Theoretical Values ΔG⁰ = -(2 mols *96485 C/mol * 1.07 J/C) = -206.48 kJ

ΔH⁰ =

ΔS⁰ =

Cell: Zn(s)| Zn2+(aq, 1M) | Cu2+(aq, 1M) | Cu(S)

ΔG° = -nFE° = ΔH° - TΔS°

ΔH° = -0.87252 J/C * 2 mols * 96485 C/mol = -168,370.1844 J  -168.4kJ

ΔS° = -0.4069 x 10-3 J/C * 2 mols * 96485 C/mol = 78.52 J

ΔG° = -168,370.54 J – (298*78.52 J) = -191768.96 J = -191.77 kJ

Theoretical Values ΔG⁰ = - (2 mols * 96485 C/mol * 1.10 J/C) = -212.267 kJ

ΔH⁰ =

ΔS⁰ =

** Can someone please help calculate the theoretical ΔS⁰ and ΔH⁰ for both equations. Please show work, thanks!

Answer 1

Part 1:

Theoretical ΔH^o = -157.04 kJ.

ΔS^o = 165.89 J.

Explanation:

The theoretical ΔG^o has been obtained using the relation ΔG° = -nFE°.

The relation between ΔS^o and E° is:

             

Hence the theoretical value for ΔS^o will be this, which is given here to be 165.89 J.

Since the ΔS^o value is given, we can obtain ΔH^o value from the relation:

ΔH^o = ΔG^o(theoretical) + T ΔS^o

           = -206.48 + (298 * 0.16589) = -157.04 kJ

Part 2:

Theoretical ΔH^o = -188.87 kJ.

ΔS^o = 78.52 J.

Explanation:

Here ΔS^o = 78.52 J, which will also be the theoretical ΔS^o value.

Theoretical ΔH^o = ΔG^o(theoretical) + T ΔS^o

                                                = -212.267 kJ + (298 * 0.07852) = -188.87 kJ.