In the reaction AB_{(g)} + CD_{(g)} rightleft | vedclass

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(D) The balanced chemical equation is: $AB_{(g)} + CD_{(g)} \rightleftharpoons AD_{(g)} + CB_{(g)}$Initial moles: $1 \quad 1 \quad 0 \quad 0$Moles at

Vedclass · Accepted Answer

$9$

Vedclass · Answer

(D) The balanced chemical equation is: $AB_{(g)} + CD_{(g)} ightleftharpoons AD_{(g)} + CB_{(g)}$Initial moles: $1 \quad 1 \quad 0 \quad 0$Moles at equilibrium: $(1 - 3/4) \quad (1 - 3/4) \quad 3/4 \quad 3/4$Equilibrium moles: $1/4 \quad 1/4 \quad 3/4 \quad 3/4$Since the volume is constant,the concentration is proportional to the number of moles. The equilibrium constant $K_c$ is given by:$K_c = \frac{[AD][CB]}{[AB][CD]} = \frac{(3/4) 	imes (3/4)}{(1/4) 	imes (1/4)} = \frac{9/16}{1/16} = 9$

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