The equilibrium constant (Kc) for the reaction N2g+O2g⇌ 2NOg at temperature T is 4 × 10-4. The value of Kc, for the reaction, NOg⇌ 2NOg at temperature T is 4 × 10-4. The value of Kc,for the reaction, NOg⇌ 1/2N2g+1/2O2g at the same temperature is

We haveN2g+O2g⇌ 2NOg: Kc1=NO2N2O2NOg⇌ 1/2N2g+1/2O2g Kc2=N21/2O21/2NOObviously, Kc2=1Kc1=14×10−4=12×10−2=50.0

The equilibrium constant (Kc) for the reaction N2g+O2g⇌ 2NOg at temperature T is 4 × 10-4. The value of Kc, for the reaction, NOg⇌ 2NOg at temperature T is 4 × 10-4. The value of Kc,for the reaction, NOg⇌ 1/2N2g+1/2O2g at the same temperature is

We haveN2g+O2g⇌ 2NOg: Kc1=NO2N2O2NOg⇌ 1/2N2g+1/2O2g Kc2=N21/2O21/2NOObviously, Kc2=1Kc1=14×10−4=12×10−2=50.0

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The equilibrium constant (K_c) for the reaction $N_{2} (g) + O_{2} (g) \underset{}{⇌} 2 NO (g)$ at temperature T is 4 × 10^-4. The value of K_c, for the reaction, $NO (g) \underset{}{⇌} 2 NO (g)$ at temperature T is 4 × 10^-4. The value of K_c,for the reaction, $NO (g) \underset{}{⇌} (1 / 2) N_{2} (g) + (1 / 2) O_{2} (g)$ at the same temperature is

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0.02

2.5 × 10²

4 × 10^-4

50.0

answer is D.

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Detailed Solution

We have

$\begin{array}{l} N_{2} (g) + O_{2} (g) \underset{}{⇌} 2 NO (g) : K_{c 1} = \frac{{[NO]}^{2}}{[N_{2}] [O_{2}]} \\ NO (g) \underset{}{⇌} (1 / 2) N_{2} (g) + (1 / 2) O_{2} (g) K_{c 2} = \frac{{[N_{2}]}^{1 / 2} {[O_{2}]}^{1 / 2}}{[NO]} \end{array}$

Obviously, $K_{c 2} = \frac{1}{\sqrt{K_{c 1}}} = \frac{1}{\sqrt{4 \times 10^{- 4}}} = \frac{1}{2 \times 10^{- 2}} = 50 .0$

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The equilibrium constant (Kc) for the reaction N2g+O2g⇌ 2NOg at temperature T is 4 × 10-4. The value of Kc, for the reaction, NOg⇌ 2NOg at temperature T is 4 × 10-4. The value of Kc,for the reaction, NOg⇌ 1/2N2g+1/2O2g at the same temperature is

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