A voltaic cell or galvanic cell converts chemical energy to electrical energy. $E _ { \text {cell } } ^ { \circ }$ for the given galvanic cell is -1.80 V. Fe²⁺(aq) + 2 Cl^-(aq) ? Fe(s) + Cl₂(g)
Calculate the value of ?_rG° for the reaction.

Question

A voltaic cell or galvanic cell converts chemical energy to electrical energy.

E _ { \text {cell } } ^ { \circ }

for the given galvanic cell is -1.80 V. Fe²⁺(aq) + 2 Cl^-(aq) ? Fe(s) + Cl₂(g)
Calculate the value of ?_rG° for the reaction.

Quizplus · Accepted Answer

The standard Gibbs free energy change ($ \Delta_r G^\circ $) can be calculated using the formula: $ \Delta_r G^\circ = -nFE^\circ_{\text{cell}} $. Here, $ n = 2 $ (number of moles of electrons transferred), $ F = 96485 \, \text{C/mol} $, and $ E^\circ_{\text{cell}} = -1.80 \, \text{V} $. Substituting these values gives $ \Delta_r G^\circ = -2 \times 96485 \times (-1.80) = 347 \, \text{kJ/mol} $.

A Voltaic Cell or Galvanic Cell Converts Chemical Energy to Electrical