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

The correct option is A 3.3 × 10^ 3 mol litre^ 1 N _ 2 O _ 4 ⇌ 2 NO _ 2 K _ C =[ NO _ 2 ] #160; ^ 2 [ N _ 2 O _ 4 ] #160; = 1.2× 10 ^ ...

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Byju's Answer

Standard XII

Chemistry

Elementary and Complex Reactions

For the react...

Question

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

3.3 \times 10^{- 3} m o l l i t r e^{- 1}

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3 \times 10^{1} m o l l i t r e^{- 1}

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3 \times 10^{- 3} m o l l i t r e^{- 1}

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3 \times 10^{3} m o l l i t r e^{- 1}

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Solution

The correct option is A $3.3 \times 10^{- 3} m o l l i t r e^{- 1}$
$N_{2} O_{4} ⇌ 2 {N O}_{2}$
$K_{C} = \frac{{[{N O}_{2}]}^{2}}{[N_{2} O_{4}]} = \frac{1.2 \times 10^{- 2} \times 1.2 \times 10^{- 2}}{4.8 \times 10^{- 2}} = 3 \times 10^{- 3} m o l {L i t}^{- 1}$

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Similar questions

Q. For the reaction at equilibrium:

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

, the concentration of

N_{2} O_{4}

and

N O_{2}

at equilibrium are

4.8 \times 10^{- 2}

and

1.2 \times 10^{- 2}

mol/L respectively. The value of

K_{c}

for the reaction is:

Q. For a 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

respectively. The value of

K_{c}

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Q. For the reaction at equilbrium:

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

, the concentration of

N_{2} O_{4}

and

N O_{2}

at equilibrium are

4.8 \times 10^{- 2}

and

1.2 \times 10^{- 2} mol/L

respectively. The value of

K_{c}

for the reaction is:

Q. For the reaction in 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 this reaction is:

Q. Find moles of

N_{2} O_{4}

and

N O_{2}

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1

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respectively total pressure at equilibrium is

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. Find

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N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

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

The correct option is A 3.3×10−3 mol litre−1N2O4⇌2NO2KC=[NO2]2[N2O4]=1.2×10−2×1.2×10−24.8×10−2=3×10−3molLit−1

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

The correct option is A $3.3 \times 10^{- 3} m o l l i t r e^{- 1}$
$N_{2} O_{4} ⇌ 2 {N O}_{2}$
$K_{C} = \frac{{[{N O}_{2}]}^{2}}{[N_{2} O_{4}]} = \frac{1.2 \times 10^{- 2} \times 1.2 \times 10^{- 2}}{4.8 \times 10^{- 2}} = 3 \times 10^{- 3} m o l {L i t}^{- 1}$