The equilibrium constant for the reaction N_2(g) + O_2(g) leftharpoons 2NO(g) at temperature T is 4 × 10^-4 . The value of K_c for the reaction NO(g) - Chemistry MCQ AIEEE 2004 2026 | ExamTest.live

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

Solution & Step-by-step Explanation

Let K_{1} be the constant for the first reaction: K_{1} = \frac{[ NO ] ^{2}}{[ N _{2} ] [ O _{2} ]} = 4 \times 1 0^{- 4} . The second reaction is the reverse of the first, divided by 2 . K_{2} = \frac{[ N _{2} ] ^{1/2} [ O _{2} ] ^{1/2}}{[ NO ]} . This is equal to \frac{1}{K _{1}} . K_{2} = \frac{1}{4 \times 1 0 ^{- 4}} = \frac{1 0 ^{4}}{4} = \frac{100}{2} = 50 .

Try it yourself before checking the explanation above.

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

2.5 \times 1 0^{2}

0.02

4 \times 1 0^{- 4}

50

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