Question

What is the ΔG⁰ for the following reaction?

\[\ce{Al_{(s)} + Fe^{3+}_{( aq)} -> Al^{3+}_{( aq)} + Fe_{(s)}}\]; \[\ce{E^0_{cell}}\] = +2.43

Options

• −703 kJ

• −469 kJ

• −235 kJ

• −173 kJ

Answer 1

−703 kJ

Explanation:

For the reaction, n = 3.

ΔG⁰ = −n F `"E"_"cell"^0`

= −3 × 96500 × 2.43

= −703485 J

= −703 kJ