The equilibrium constant (Kc) for the reaction N2(g)+O2(g)→2NO(g) at temperature T is 4×10−4. The value of Kc for the reaction, NO(g) → ½ N2(g) + ½ O2(g) at the same temperature is

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The equilibrium constant {({K}_{{{c}}})} for the reaction {N}_

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The equilibrium constant $(K_{c})$ for the reaction $N_{2} (g) + O_{2} (g) \to 2 N O (g)$ at temperature T is $4 \times 10^{- 4}$ . The value of $K_{c}$ for the reaction, NO(g) $\to$ ½ $N_{2} (g)$ + ½ $O_{2} (g)$ at the same temperature is

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The equilibrium constant

(K_{c})

for the reaction

N_{2} (g) + O_{2} (g) \to 2 N O (g)

at temperature T is

4 \times 10^{- 4}

. The value of

K_{c}

for the reaction, NO(g)

\to

N_{2} (g)

+ ½

O_{2} (g)

at the same temperature is

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Question Text	The equilibrium constant $(K_{c})$ for the reaction $N_{2} (g) + O_{2} (g) \to 2 N O (g)$ at temperature T is $4 \times 10^{- 4}$ . The value of $K_{c}$ for the reaction, NO(g) $\to$ ½ $N_{2} (g)$ + ½ $O_{2} (g)$ at the same temperature is
Answer Type	Video solution: 1
Upvotes	151