At constant temperature- Kp for the equilibrium N2O4-2NO2 is expressed by Kp-4X2P1-X2- where P-pressure-X-degree of dissociation-Which of the following statements is false-

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Standard XII

Chemistry

Dalton's Law of Partial Pressures

At constant t...

Question

At constant temperature, $K_{p}$ for the equilibrium $N_{2} O_{4} ⇌ 2 N O_{2}$ is expressed by $K_{p} = \frac{4 X^{2} P}{1 - X^{2}}$ , where P=pressure,X=degree of dissociation.Which of the following statements is false?

K_{p}

increases with increase of P

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K_{p}

increases with increase of X

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K_{p}

remains constant with change in temperature

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All of these

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Solution

The correct option is A $K_{p}$ increases with increase of P
Option C is false
$K_{p} = \frac{4 \times^{2} P}{1 - X^{2}} \begin{matrix} K_{P} ↑_{e s} w h e n P ↑_{e s} K_{P} ↑_{e s} w h e n X ↑_{e s} \end{matrix}$
When X increases numerator increases.
and denominator decrease so Kp increases.

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Similar questions

Q. At constant temperature, the equilibrium constant

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Is expressed by

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Where P = pressure, x = extent of decomposition. Which one of the following statements are false?

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At constant temperature, Kp for the equilibrium N2O4⇌2NO2 is expressed by Kp=4X2P1−X2, where P=pressure,X=degree of dissociation.Which of the following statements is false?

The correct option is A Kp increases with increase of POption C is falseKp=4×2P1−X2KP↑eswhenP↑esKP↑eswhenX↑esWhen X increases numerator increases.and denominator decrease so Kp increases.

At constant temperature, $K_{p}$ for the equilibrium $N_{2} O_{4} ⇌ 2 N O_{2}$ is expressed by $K_{p} = \frac{4 X^{2} P}{1 - X^{2}}$ , where P=pressure,X=degree of dissociation.Which of the following statements is false?