AP EAMCET · Chemistry · Chemical Equilibrium
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?
- A \(2 \times 10^{-4}\)
- B \(10^{-4}\)
- C \(2 \times 10^4\)
- D \(10^4\)
Answer & Solution
Correct Answer
(A) \(2 \times 10^{-4}\)
Step-by-step Solution
Detailed explanation
\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…
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