At , the equilibrium constant for Reaction 1 is . Reaction 1: Reaction 2 is the…

CHEMISTRY · Subjective · A Level · Chemistry · Thermodynamics · Thermodynamics

Problem

298\,\text{K}

, the equilibrium constant for Reaction 1 is

K_1 = 8.0 \times 10^6

. Reaction 1:

\mathrm{C_2H_4(g)} + \mathrm{H_2(g)} \rightleftharpoons \mathrm{C_2H_6(g)}

Reaction 2 is the reverse process (

\mathrm{C_2H_6} \rightleftharpoons \mathrm{C_2H_4} + \mathrm{H_2}

). Calculate the standard Gibbs free energy change,

\Delta G^\circ

(in

\text{kJ mol}^{-1}

), for Reaction 2 at

298\,\text{K}

. (Use

R = 8.314\,\text{J mol}^{-1}\,\text{K}^{-1}