Home
Class 11
CHEMISTRY
At constant temperature, the equilibrium...

At constant temperature, the equilibrium constant `(K_(p))` for the decomposition reaction
`N_(2)O_(4) hArr 2NO_(2)`
is expressed by `K_(p)=4x^(2)p//(1-x^(2))`, where p=pressure x= extent of decomposition. Which of the following statements is true?

A

`K_(P)` increases with increase of `P`

B

`K_(P)` increases with increase of `x`

C

`K_(P)` increases with decrease of `x`

D

`K_(P)` remains constant with change in `P "and" x`

Text Solution

Verified by Experts

The correct Answer is:
D
With change of pressure, `x` will change in such a way that `K_(P)` remains a constant.
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    RESONANCE|Exercise Exercise-3 (Part-2)|17 Videos

  • CHEMICAL EQUILIBRIUM

    RESONANCE|Exercise Advanced Level Problems (Part-1)|31 Videos

  • CHEMICAL EQUILIBRIUM

    RESONANCE|Exercise Exercise-2 (Part-4)|6 Videos

  • CHEMICAL BONDING

    RESONANCE|Exercise Inorganic chemistry (Chemistry Bonding)|49 Videos

  • D & F-BLOCK ELEMENTS & THEIR IMPORTANT COMPOUNDS

    RESONANCE|Exercise Match the column|1 Videos

Similar Questions

Explore conceptually related problems

At constant temperature, the equilibrium constant (K_(p)) for the decomopsition reaction N_(2)O_(4)hArr2NO_(2) is expressed by K_(p) = ((4x^(2)P))/((1-x^(2)) , where P = pressure, x = extent of decomposition. Which one of the following statement is true ?