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(A) The reaction $A_{(g)} ightleftharpoons B_{(g)} + 	ext{Heat}$ is exothermic. According to Le Chatelier's principle,exothermic reactions are favo

Vedclass · Accepted Answer

$A-ii, B-iii, C-i, D-v, E-iv$

Vedclass · Answer

(A) The reaction $A_{(g)} ightleftharpoons B_{(g)} + 	ext{Heat}$ is exothermic. According to Le Chatelier's principle,exothermic reactions are favored at low temperatures. So,$A-ii$.$(B)$ The ratio of the rate of backward reaction to the rate of forward reaction $(r_b/r_f)$ is equal to the inverse of the equilibrium constant $(K_c^{-1})$. So,$B-iii$.$(C)$ The ratio of the rate of forward reaction to the rate of backward reaction $(r_f/r_b)$ is equal to the equilibrium constant $(K_c)$. So,$C-i$.$(D)$ For the reaction $2A_{(g)} + B_{(g)} ightleftharpoons C_{(g)}$,the change in moles of gas is $\Delta n = 1 - (2+1) = -2$. Since $\Delta n $(E)$ The effect of pressure is significant when $\Delta n 
eq 0$. The reaction $A_{(g)} + B_{(g)} ightleftharpoons C_{(g)} + D_{(g)}$ has $\Delta n = (1+1) - (1+1) = 0$,meaning pressure has no effect. However,in the context of the options provided,$E$ corresponds to the reaction where pressure change is relevant or the general principle. Given the options,$E-iv$ is the intended match as it represents a system where pressure change is discussed. Therefore,the correct sequence is $A-ii, B-iii, C-i, D-v, E-iv$.

List-$X$	List-$Y$
$(A)$ $A_{(g)} \rightleftharpoons B_{(g)} + \text{Heat}$	$(i)$ Equilibrium constant
$(B)$ $r_b/r_f$	$(ii)$ Favored at low temperature
$(C)$ $r_f/r_b$	$(iii)$ [Equilibrium constant]$^{-1}$
$(D)$ $2A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)}$	$(iv)$ $A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$
$(E)$ Effect of pressure	$(V)$ $\Delta n < 0$

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