In the reaction A_{(g)} + 2B_{(g)} rightlefth | vedclass

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(C) The given reaction is $A_{(g)} + 2B_{(g)} \rightleftharpoons C_{(g)} + Q \ kJ$. Since heat $(Q)$ is released,the reaction is exothermic,meaning $\

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At low temperature and high pressure

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(C) The given reaction is $A_{(g)} + 2B_{(g)} \rightleftharpoons C_{(g)} + Q \ kJ$. Since heat $(Q)$ is released,the reaction is exothermic,meaning $\Delta H According to Le Chatelier's principle,for an exothermic reaction,a low temperature favors the forward direction. For the pressure effect,we look at the change in the number of moles of gaseous species: $\Delta n_g = n_p - n_r = 1 - (1 + 2) = -2$. Since $\Delta n_g Therefore,high pressure and low temperature favor the forward reaction.

In the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons C_{(g)} + Q \ kJ$,greater product will be obtained or the forward reaction is favoured by:

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