WBJEE · Chemistry · Chemical Equilibrium
The following equilibrium constants are given
\(\begin{array}{l}
\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3} ; K_{1} \\
\mathrm{N}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{NO} ; K_{2}
\end{array}\)
\(\mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightleftharpoons \mathrm{H}_{2} \mathrm{O} ; K_{3}\)
The equilibrium constant for the oxidation of 2 mole of \(\mathrm{NH}_{3}\) to give NO is
- A \(K_{1} \cdot \frac{K_{2}}{K_{3}}\)
- B \(K_{2} \cdot \frac{K_{3}^{3}}{K_{1}}\)
- C \(K_{2}, \frac{K_{2}^{2}}{K_{1}}\)
- D \(K_{2}^{2} \frac{K_{3}}{K_{1}}\)
Answer & Solution
Correct Answer
(B) \(K_{2} \cdot \frac{K_{3}^{3}}{K_{1}}\)
Step-by-step Solution
Detailed explanation
\begin{array}{l} \text {Given, } \\ \begin{aligned} \mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3} ; K_{1} &=\frac{\left[\mathrm{NH}_{3}\right]^{2}}{\left[\mathrm{N}_{2}\right]\left[\mathrm{H}_{2}\right]^{3}} \\ \mathrm{N}_{2}+\mathrm{O}_{2}…
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