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The yield of the product in the reaction
$$
\mathrm{A}_{2}(\mathrm{~g})+2 \mathrm{~B}(\mathrm{~g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{Q} \mathrm{kJ}
$$
would be higher at
Options:
$$
\mathrm{A}_{2}(\mathrm{~g})+2 \mathrm{~B}(\mathrm{~g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{Q} \mathrm{kJ}
$$
would be higher at
Solution:
2636 Upvotes
Verified Answer
The correct answer is:
low temperature and high pressure
$A_{2}(g)+2 B(g) \rightleftharpoons C(g)+Q k J$ Since, the reaction is exothermic, So, it is favoured by low temperature.
In addition, the number of moles of products is lesser than the number of moles of reactants, thus high pressure favours the forward reaction.
In addition, the number of moles of products is lesser than the number of moles of reactants, thus high pressure favours the forward reaction.
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