Question

For the given reaction, \[ H_2(g) + Cl_2(g) \rightleftharpoons 2HCl(aq) + 2ClT(aq); \, \Delta G = -262kJ \] The value of free energy of formation (\( \Delta G_f \)) for the ion C\( T_1 \) is

• A. \( -131.2 \, \text{kJ mol}^{-1} \)
• B. \( +131.2 \, \text{kJ mol}^{-1} \)
• C. \( -262.4 \, \text{kJ mol}^{-1} \)
• D. \( +262.4 \, \text{kJ mol}^{-1} \)

Hint:

The free energy of formation for a substance is calculated by dividing the total free energy change by the number of molecules involved.

Answer 1

The Correct Option is B

The free energy of formation is half of \( \Delta G \) for a molecule involving two ions, so \( \Delta G_f \) for C\( T_1 \) is \( +131.2 \, \text{kJ mol}^{-1} \).