In a system A_{(s)} rightleftharpoons 2B_{(g) | vedclass

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(D) The equilibrium constant expression for the reaction $A_{(s)} \rightleftharpoons 2B_{(g)} + 3C_{(g)}$ is given by $K_{c} = [B]^{2}[C]^{3}$.Let the

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$\frac{1}{2\sqrt{2}}$ times the original value

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(D) The equilibrium constant expression for the reaction $A_{(s)} ightleftharpoons 2B_{(g)} + 3C_{(g)}$ is given by $K_{c} = [B]^{2}[C]^{3}$.Let the initial equilibrium concentrations be $[B]$ and $[C]$.When the concentration of $C$ is increased by a factor of $2$,the new concentration becomes $[C'] = 2[C]$.Since $K_{c}$ remains constant at a constant temperature,let the new concentration of $B$ be $[B']$.$K_{c} = [B]^{2}[C]^{3} = [B']^{2}[C']^{3}$.$[B]^{2}[C]^{3} = [B']^{2}(2[C])^{3}$.$[B]^{2}[C]^{3} = [B']^{2} 	imes 8[C]^{3}$.$[B]^{2} = 8[B']^{2}$.$[B']^{2} = \frac{[B]^{2}}{8}$.$[B'] = \frac{[B]}{\sqrt{8}} = \frac{1}{2\sqrt{2}}[B]$.

In a system $A_{(s)} \rightleftharpoons 2B_{(g)} + 3C_{(g)},$ if the concentration of $C$ at equilibrium is increased by a factor of $2,$ it will cause the equilibrium concentration of $B$ to change to

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