The equilibrium constant ( K_c ) for the reaction N_2(g) + O_2(g) → 2NO(g) at temperature T is 4 × 10^-4 . The value of K_c for the reaction, NO(g) → - Chemistry MCQ AIEEE 2012 2026 | ExamTest.live

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The equilibrium constant (K_{c}) for the reaction N_{2} (g) + O_{2} (g) \to 2 NO(g) at temperature T is 4 \times 1 0^{- 4} . The value of K_{c} for the reaction, NO(g) \to \frac{1}{2} N_{2} (g) + \frac{1}{2} O_{2} (g) at the same temperature is:

Solution & Step-by-step Explanation

Original reaction: N_{2} + O_{2} \to 2 NO (K_{c} = 4 \times 1 0^{- 4}).Target reaction is the reverse of the original, divided by 2.Reverse the reaction: 2 NO \to N_{2} + O_{2} (K^{'} = \frac{1}{K _{c}} = \frac{1}{4 \times 1 0 ^{- 4}} = 2500).Divide by 2: NO \to \frac{1}{2} N_{2} + \frac{1}{2} O_{2} (K^{''} = K^{'} = 2500 = 50.0).

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The equilibrium constant (K_{c}) for the reaction N_{2} (g) + O_{2} (g) \to 2 NO(g) at temperature T is 4 \times 1 0^{- 4} . The value of K_{c} for the reaction, NO(g) \to \frac{1}{2} N_{2} (g) + \frac{1}{2} O_{2} (g) at the same temperature is:

0.02

2.5 \times 1 0^{2}

4 \times 1 0^{- 4}

50.0

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