(A) The given reaction is $A_{2(g)} + B_{2(g)} \rightleftharpoons X_{2(g)}$.$1$. The enthalpy change $\Delta_{r} H = -X \ kJ$ indicates that the react

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Low temperature and high pressure

(A) The given reaction is $A_{2(g)} + B_{2(g)} \rightleftharpoons X_{2(g)}$.$1$. The enthalpy change $\Delta_{r} H = -X \ kJ$ indicates that the reaction is exothermic $(\Delta H $2$. The change in the number of gaseous moles is $\Delta n_{g} = n_{p} - n_{r} = 1 - (1 + 1) = -1$. Since $\Delta n_{g} Therefore,low temperature and high pressure favour the maximum formation of the product.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Le-Chaterlier principle and It’s application

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Which one of the following conditions will favour maximum formation of the product in the reaction
$A_{2(g)} + B_{2(g)} \rightleftharpoons X_{2(g)}; \Delta_{r} H = -X \ kJ$

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Low temperature and high pressure
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Low temperature and low pressure
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High temperature and high pressure
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High temperature and low pressure

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

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Which one of the following conditions will favour maximum formation of the product in the reaction$A_{2(g)} + B_{2(g)} \rightleftharpoons X_{2(g)}; \Delta_{r} H = -X \ kJ$

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Which one of the following conditions will favour maximum formation of the product in the reaction
$A_{2(g)} + B_{2(g)} \rightleftharpoons X_{2(g)}; \Delta_{r} H = -X \ kJ$