Chemistry · THERMODYNAMICS

For the reaction \( 2\text{NH}_3(g) + \text{CO}_2(g) \rightleftharpoons \text{NH}_2\text{CONH}_2(aq) + \text{H}_2\text{O}(l) \) at \( 298\text{ K} \), \( \Delta_r G^\circ = -13.6\text{ kJ mol}^{-1} \). Find the equilibrium constant \( K \). (Given: \( \frac{13.6 \times 10^3}{2.303 \times 8.314 \times 298} = 2.38 \) and \( 10^{0.38} = 2.4 \))

1. \( 2.4 \times 10^{-2} \)
2. \( 4.8 \times 10^{2} \)
3. \( 1.2 \times 10^{3} \)
4. \( 2.4 \times 10^{2} \)