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Half life

At constant t...

Question

At constant temperature, the equilibrium constant ( $K_{p})$ for the decomposition reaction,
$N_{2} O_{4} ⇌ 2 {N O}_{2}$
is expressed by:
$K_{p} = \frac{4 x^{2} P}{(1 - x^{2})}$
Where, $P =$ pressure, $x =$ extent of decomposition. Which one of the following statements is true?

A

K_{p}

increases with increase of

P

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B

K_{p}

increases with increase of

x

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C

K_{p}

increases with decrease of

x

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D

K_{p}

remains constant with change in

P

and

x

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Solution

The correct option is D $K_{p}$ remains constant with change in $P$ and $x$
At constant temperature, the equilibrium constant ( $K_{p})$ for the decomposition reaction,
$N_{2} O_{4} ⇌ 2 {N O}_{2}$
is expressed by:
$K_{p} = \frac{4 x^{2} P}{(1 - x^{2})}$
Where, $P =$ pressure, $x =$ extent of decomposition. The following statement is true.
(D) $K_{p}$ remains constant with change in $P$ and $x$
The value of the equilibrium constant depends on temperature. It is not affected by changes in concentration, pressure, extent of dissociation or presence of catalyst.

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