Consider the following reaction: 2A(g) + B(g) arrow 2D(g)$$2A(g) + B(g) \rightarrow 2D(g)$$ Δ U° = -10 kJ mol⁻¹ and Δ S° = -44 J K⁻¹ at 298 K$$\Delta U^{\circ} = -10 \text{ kJ mol}^{-1} \quad \text{and} \quad \Delta S^{\circ} = -44 \text{ J K}^{-1} \text{ at } 298 \text{ K}$$ Identify the correct option with Δ G°$\Delta G^{\circ}$ for the reaction and spontaneity of the reaction at 298 K. (Given: R = 8.31 J mol⁻¹ K⁻¹$R = 8.31 \text{ J mol}^{-1} \text{K}^{-1}$)

Related Formula

Core Logic

Heat absorbed q = +500 J$q = +500 \text{ J}$. Work done by system w = -200 J$w = -200 \text{ J}$.

Step 1: Conclusion

Change in internal energy is 300 J$300 \text{ J}$.

Pattern Recognition

First Law sign convention: heat absorbed is positive, work done by system is negative.

Chapter Mix

Class 11 Chemistry: Thermodynamics