For the reaction 2A_{(g)} + B_{(g)} rightleft | vedclass

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(C) The given reaction is $2A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + 362 \, kcal$.
Since the reaction is exothermic $(\Delta H < 0)$,accordi

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$1000 \, atm$ and $50 \, ^\circ C$

Vedclass · Answer

(C) The given reaction is $2A_{(g)} + B_{(g)} ightleftharpoons C_{(g)} + 362 \, kcal$.
Since the reaction is exothermic $(\Delta H < 0)$,according to Le Chatelier's principle,a lower temperature will shift the equilibrium to the right,favoring the formation of products.
For the pressure effect,we look at the change in the number of moles of gas: $\Delta n_g = n_{	ext{products}} - n_{	ext{reactants}} = 1 - (2 + 1) = -2$.
Since $\Delta n_g < 0$,an increase in pressure will shift the equilibrium towards the side with fewer moles of gas,which is the product side.
Therefore,high pressure and low temperature favor the formation of $C$.

For the reaction $2A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + 362 \, kcal$,which combination of pressure and temperature will favor the formation of $C$ at equilibrium?

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