JEE Main 2016 · 9 Apr · Shift 1 · Chemistry Q37

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ChemistrySingle correct+4 / -1Question 37 of 90

For the reaction, $\ce{A(g) + B(g) -> C(g) + D(g)}$ , ΔH° and ΔS° are, respectively, −29.8 kJ mol $^{-1}$ and −0.100 kJ K $^{-1}$ mol $^{-1}$ at 298 K. The equilibrium constant for the reaction at 298 K is :

1.0\times10^{-10}

1.0\times10^{10}

Answer and worked solution

Official answer: D

$\Delta G^\circ=-29.8-298(-0.100)=0$ , so $K=e^0=1$ .

Topics:Equilibrium and Gibbs energy

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JEE Main 2016 · 9 Apr · Shift 1, Chemistry question 37