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Chemistry · EQUILIBRIUM
हिन्दीAt a certain temperature, for the reaction \( \text{N}_2(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{NO}(\text{g}) \), the equilibrium concentrations are \( [\text{N}_2] = 3.0 \times 10^{-3}\text{ M} \), \( [\text{O}_2] = 4.2 \times 10^{-3}\text{ M} \), and \( [\text{NO}] = 2.8 \times 10^{-3}\text{ M} \). What is the value of the equilibrium constant \( K_c \) for the reverse reaction \( 2\text{NO}(\text{g}) \rightleftharpoons \text{N}_2(\text{g}) + \text{O}_2(\text{g}) \)?
Correct answer · Option 1
\( 1.61 \)
Explanation
For forward reaction, \( K_c = \frac{(2.8 \times 10^{-3})^2}{(3.0 \times 10^{-3})(4.2 \times 10^{-3})} = 0.622 \). For the reverse reaction, \( K'_c = \frac{1}{0.622} \approx 1.61 \).
