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Characteristics of Equilibrium Constant

For a reactio...

Question

For a reaction equilibrium, $N_{2} O_{4} (g) \to 2 N O_{2} (g)$ , the concentration of $N_{2} O_{4} (g)$ 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 for the reaction is:

A

3 \times 10^{- 3}

mol/L

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B

3.3 \times 10^{- 3}

mol/L

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C

3 \times 10^{- 1}

mol/L

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D

3.3 \times 10^{- 1}

mol/L

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Solution

The correct option is B $3 \times 10^{- 3}$ mol/L
The equilibrium constant for the given reaction is-
$K_{c} = \frac{[N O_{2}]^{2}}{[N_{2} O_{4}]}$
$K_{c} = \frac{(1.2 \times 10^{- 2} m o l / L)^{2}}{4.8 \times 10^{- 2} m o l / L}$
$K_{c} = 3 \times 10^{- 3} m o l / L$

Thus, the correct option is $A$

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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

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4.8 \times 10^{- 2}

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Q. For the reaction equilibrium

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Q. For the reaction at equilbrium:

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

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P C l_{5}, P C l_{3} a n d C l_{2}

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\begin{matrix} Experiment No. & [A] (m o l d m^{- 3}) & [B] (m o l d m^{- 3}) & [C] (m o l d m^{- 3}) & Rate of the reaction (m o l d m^{- 3} s^{- 1}) 1 & 0.2 & 0.1 & 0.1 & 6.0 \times 10^{- 5} 2 & 0.2 & 0.2 & 0.1 & 6.0 \times 10^{- 5} 3 & 0.2 & 0.1 & 0.2 & 1.2 \times 10^{- 4} 4 & 0.3 & 0.1 & 0.1 & 9.0 \times 10^{- 5} \end{matrix}

The rate of the reaction for

[A] = 0.15 m o l d m^{- 3}, [B] = 0.25 m o l d m^{- 3} a n d [C] = 0.15 m o l d m^{- 3}

Y \times 10^{- 5} m o l d m^{- 3} s^{- 1}

.The value of Y is

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