Question

If ΔH° and ΔS° for the reaction \[\ce{N2O_{4(g)} -> 2NO_{2(g)}}\] is 57.24 kJ and 175.8 JK^-1 mol^-1 respectively. What is the value of ΔG° for this reaction at 298 K?

Options

• 57.24 kJ

• - 17.58 kJ

• 4.85 kJ

• - 4.85 kJ

Answer 1

4.85 kJ

Explanation:

\[\ce{N2O_{4(g)} -> 2NO_{2(g)}}\];    ΔH° = 57.24 kJ, ΔS° = 0.1758 kJ K^-1 mol^-1

ΔG = ΔH - T Δ S

= 57.24 - 298 (0.1758)

= 4.8516 kJ