1. Tardigrade
  2. Question
  3. Chemistry
  4. At 550 K, the Kc for the following reaction is 104 mol -1 L X(g)+Y(g) leftharpoons Z(g) At equilibrium, it was observed that [X]=(1/2)[Y]=(1/2)[Z] What is the value of [Z] (in mol L -1 ) at equilibrium?

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Q. At $550\, K$, the $K_{c}$ for the following reaction is $10^{4} mol ^{-1} L$
$X_{(g)}+Y_{(g)} \rightleftharpoons Z_{(g)}$
At equilibrium, it was observed that
$[X]=\frac{1}{2}[Y]=\frac{1}{2}[Z]$
What is the value of $[Z]$ (in $mol L ^{-1}$ ) at equilibrium?

Equilibrium

Solution:

Let $[X]=\frac{1}{2}[Y]=\frac{1}{2}[Z]=x$

then $[Y]=2 x$ and $[Z]=2 x,[X]=x$

Now, $K=\frac{[Z]}{[X][Y]} $

$\Rightarrow 10^{4}=\frac{2 x}{x \times 2 x}$

$ \Rightarrow x=10^{-4}$

$\therefore [Z]=2 x=2 \times 10^{-4}$