NEET 2023 Phase 1 · ChemistryPrevious Year Question

The equilibrium concentrations of the species in the reaction $A + B C + D$ are $2$ , $3$ , $10$ and $6 mol L^{- 1}$ , respectively, at $300 K$ . $Δ G^{\circ}$ for the reaction is (Given $R = 2 cal mol^{- 1} K^{- 1}$ ).

Answer: (C) $- 1381.80 cal$ . \textbf{Answer:} (C) $- 1381.80 cal$ \textbf{Solution:} Equilibrium constant: $K = \frac{[ C ] [ D ]}{[ A ] [ B ]} = \frac{10 \times 6}{2 \times 3} = 10$ .

A. $1372.60 cal$
B. $- 137.26 cal$
C. $- 1381.80 cal$ ✓
D. $- 13.73 cal$

Correct Answer

Solution & Explanation

\textbf{Answer:} (C) $- 1381.80 cal$ \textbf{Solution:} Equilibrium constant: $K = \frac{[ C ] [ D ]}{[ A ] [ B ]} = \frac{10 \times 6}{2 \times 3} = 10$ . Then $Δ G^{\circ} = - 2.303 R T lo g K = - 2.303 \times 2 \times 300 \times lo g (10) = - 2.303 \times 2 \times 300 \times 1 = - 1381.80 cal$ . Mapped: source lowercase answer 'c' → option C.

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The equilibrium concentrations of the species in the reaction A+B​C+D are 2, 3, 10 and 6 molL−1, respectively, at 300 K. ΔG∘ for the reaction is (Given R=2 calmol−1K−1).

Solution & Explanation

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The equilibrium concentrations of the species in the reaction $A + B C + D$ are $2$ , $3$ , $10$ and $6 mol L^{- 1}$ , respectively, at $300 K$ . $Δ G^{\circ}$ for the reaction is (Given $R = 2 cal mol^{- 1} K^{- 1}$ ).