A reaction at $300 \mathrm{~K}$ with $\Delta G^{\circ}=-1743 \mathrm{~J}$ consists of 3 moles of $\mathrm{A}(\mathrm{g}),$ 6 moles of $\mathrm{B}(\mathrm{g})$ and 3 moles of $\mathrm{C}(\mathrm{g}).$ If $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ are in equilibrium in one liter vessel, then the reaction should be $(\ln 2=0.7$, $R=8.3 \mathrm{~J} / \mathrm{K}-\mathrm{mol})$

$\mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}$

$\mathrm{A} \rightleftharpoons \mathrm{B}+2 \mathrm{C}$

$\mathrm{A}+\mathrm{B} \rightleftharpoons 2 \mathrm{C}$

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NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Application +4 | -1

A reaction at

300 \mathrm{~K}

with

\Delta G^{\circ}=-1743 \mathrm{~J}

consists of 3 moles of

\mathrm{A}(\mathrm{g}),

6 moles of

\mathrm{B}(\mathrm{g})

and 3 moles of

\mathrm{C}(\mathrm{g}).

\mathrm{A}, \mathrm{B}

and

\mathrm{C}

are in equilibrium in one liter vessel, then the reaction should be

(\ln 2=0.7

R=8.3 \mathrm{~J} / \mathrm{K}-\mathrm{mol})

View answer and explanation

Correct option: C

2 \mathrm{A} \rightleftharpoons \mathrm{B}+\mathrm{C}

Option C (

2 \mathrm{A} \rightleftharpoons \mathrm{B}+\mathrm{C}

) is correct because by calculating the equilibrium constant K from the given Δ G° and comparing it with the reaction quotient Q, we can determine that the reaction shifts towards the products, which corresponds to the stoichiometry of the reaction

2 \mathrm{A} \rightleftharpoons \mathrm{B}+\mathrm{C}

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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