At 298K, the equilibrium constant for a reaction $\large {A_{\left( g \right)}} + {B_{\left( g \right)}}\, \rightleftharpoons \,{C_{\left( g \right)}} + {D_{\left( g \right)}}$ is 100. If the initial concentration of each species is 1M, the equilibrium concentration of D in molL^-¹ is

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0.818

1.182

1.818

0.182

answer is B.

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Detailed Solution

Given

$1 + x = 10 - 10 x; x = \frac{9}{11}; {[D]}_{eq} = 1 + x; {[D]}_{eq} = 1 + \frac{9}{11} = 1.818 M;$

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Stoichiometry	$\large \mathop {A\left( g \right)}\limits^{1{\text{ }}mole} +$	$\large \mathop {B\left( g \right)}\limits^{1{\text{ }}mole}$	$\large \rightleftharpoons$	$\large \mathop {C\left( g \right)}\limits^{1{\text{ }}mole} +$	$\large \mathop {D\left( g \right)}\limits^{1{\text{ }}mole};K_C=100$
Initial concentration	1M	1M		1M	1M
Equilibrium concentration	(1 - x)	(1 - x)		(1 + x)	(1 + x)