NEET 2026 — Chemistry solution

NEET2026Chemistry

Consider the following reaction :

$2 A (g) + B (g) \to 2 D (g)$

$Δ U^{\circ} = - 10$ kJ mol $^{- 1}$ and $Δ S^{\circ} = - 44$ J K $^{- 1}$ at 298 K.

Identify the correct option with $Δ G^{\circ}$ for the reaction and spontaneity of the reaction at 298 K.

(Given : R = 8.31 J mol $^{- 1}$ K $^{- 1}$ )

Solution

$Δ n_{g} = 2 - 3 = - 1$ .

$Δ H^{\circ} = Δ U^{\circ} + Δ n_{g} R T = - 10 + \frac{( - 1 ) ( 8.31 ) ( 298 )}{1000} = - 10 - 2.4734 = - 12.4734$ kJ mol $^{- 1}$ .

$Δ G^{\circ} = Δ H^{\circ} - T Δ S^{\circ} = - 12.4734 - \frac{298 \times ( - 44 )}{1000} = - 12.4734 + 13.112 = + 0.6386$ kJ mol $^{- 1}$ .

Since $Δ G^{\circ} > 0$ , the reaction is non-spontaneous.

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