Search any question & find its solution
Question:
Answered & Verified by Expert
At $550 \mathrm{~K}$, the $K_c$ for the following reaction is $10^4 \mathrm{~mol}^{-1} \mathrm{~L} X(g)+Y(g) \rightleftharpoons Z(g)$
At equilibrium, it was observed that $[X]=\frac{1}{2}[Y]=\frac{1}{2}[Z]$
What is the value of [Z] (in $\mathrm{mol} \mathrm{L}^{-1}$ ) at equilibrium?
Options:
At equilibrium, it was observed that $[X]=\frac{1}{2}[Y]=\frac{1}{2}[Z]$
What is the value of [Z] (in $\mathrm{mol} \mathrm{L}^{-1}$ ) at equilibrium?
Solution:
1548 Upvotes
Verified Answer
The correct answer is:
$2 \times 10^{-4}$
$\begin{aligned} & X(g)+Y(g) \rightleftharpoons Z(g) \\ & K_c=\frac{[Z]}{[X][Y]} \text { or } 10^4=\frac{[Z]}{[X][Y]} \\ & \therefore \quad[Z]=10^4[X][Y]=10^4 \times \frac{1}{2}[Z][Z] \\ & \text { (Given, }[X]=\frac{1}{3}[Y]=\frac{1}{2}[Z] \text { ) } \\ & \therefore \quad[Z]=2 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \\ & \end{aligned}$
Looking for more such questions to practice?
Download the MARKS App - The ultimate prep app for IIT JEE & NEET with chapter-wise PYQs, revision notes, formula sheets, custom tests & much more.