For the reaction equilibrium N2O4g - 2NO2g the concentrations of N2O4 and NO2 at equilibrium are 4-8 - 10-2 and 1-2 - 10-2 mol L-1 respectively- The value of Kc for the reaction is

The reaction equilibrium nbsp; N_2O_4(g) ⇌ 2NO_2(g) At equilibrium [N_2O_4]=4.8 × 10^ 2 mol L^ 1 and [NO_2]=1.2 × 10^ 2 mol L^ 1 nbsp; K_c = [NO_2]^2[N_2O_4 ...

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Standard XII

Chemistry

Elementary and Complex Reactions

For the react...

Question

For the reaction equilibrium
$N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$ the concentrations of $N_{2} O_{4}$ and $N O_{2}$ at equilibrium are $4.8 \times 10^{- 2}$ and $1.2 \times 10^{- 2} m o l L^{- 1}$ respectively. The value of $K_{c}$ for the reaction is

3 \times 10^{- 1} m o l L^{- 1}

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3 \times 10^{- 3} m o l L^{- 1}

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3 \times 10^{3} m o l L^{- 1}

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3.3 \times 10^{2} m o l L^{- 1}

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Solution

The correct option is B $3 \times 10^{- 3} m o l L^{- 1}$
The reaction equilibrium
$N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$
At equilibrium
$[N_{2} O_{4}] = 4.8 \times 10^{- 2} m o l L^{- 1}$ and $[N O_{2}] = 1.2 \times 10^{- 2} m o l L^{- 1}$
$K_{c} = \frac{[N O_{2}]^{2}}{[N_{2} O_{4}]} = \frac{[1.2 \times 10^{- 2}]^{2}}{[4.8 \times 10^{- 2}]}$
$K_{c} = 3 \times 10^{- 3} m o l L^{- 1}$

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Elementary and Complex Reactions

Standard XII Chemistry

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For the reaction equilibrium N2O4(g)⇌2NO2(g) the concentrations of N2O4 and NO2 at equilibrium are 4.8×10−2 and 1.2×10−2 mol L−1 respectively. The value of Kc for the reaction is

The correct option is B 3×10−3 mol L−1The reaction equilibrium N2O4(g)⇌2NO2(g) At equilibrium [N2O4]=4.8×10−2 mol L−1 and [NO2]=1.2×10−2 mol L−1 Kc=[NO2]2[N2O4]=[1.2×10−2]2[4.8×10−2] Kc=3×10−3 mol L−1

For the reaction equilibrium
$N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$ the concentrations of $N_{2} O_{4}$ and $N O_{2}$ at equilibrium are $4.8 \times 10^{- 2}$ and $1.2 \times 10^{- 2} m o l L^{- 1}$ respectively. The value of $K_{c}$ for the reaction is