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For the reaction, N(2(g))+ O(2(g)) Leftr...

For the reaction, `N_(2(g))+ O_(2(g)) Leftrightarrow 2NO_((g))` the value of `K_c" at "800^@C` is 0.1. When the equilibrium concentration of both the reactants is 0.5 mol, what is the value of `K_p` at this temperature?

A

0.01

B

0.5

C

0.025

D

0.1

Text Solution

Verified by Experts

The correct Answer is:
D
`N_(2(g)) +O_(2(g)) Leftrightarrow 2NO_(g)`
Applying `K_(p)=K_(c) (RT)^(trianglen_(g)) , trianglen_(g)=2-(1+1) =0 therefore K_(p)=K_(c)=0.1`
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