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For the reversible reaction N(2)(g)+3H...

For the reversible reaction
`N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)`
at `500^(@)C`, the value of `K_(p)` is `1.44xx10^(-5)` when the partial pressure is measured in atmosphere. The corresponding value of `K_(c)` with concentration in mol `L^(-1)` is

A

`1.44xx10^(-5)//(0.082xx500)^(-2)`

B

`1.44xx10^(-5)//(8.314xx773)^(-2)`

C

`1.44xx10^(-5)//(0.082xx773)^(2)`

D

`1.44xx10^(-5)//(0.082xx773)^(-2)`

Text Solution

Verified by Experts

The correct Answer is:
D
`K_(c)=K_(p)(RT)^(-Deltan_(g))`
Since `Deltan_(g)=-2`
`therefore K_(c)=1.44xx10^(-5)//(0.082xx773)^(-2)`
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For the reversible reaction N_(2)(g)+3H_(2)(g)hAr2NH_(3)(g) at 500^(@)C the value of K_(p) is 1.44xx10^(-5) when partial pressure is measured in atmosphere. The corresponding value of K_(e) with concentration in mol/L is

For the reversible reaction, N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g) At 500^(@)C , the value of Kp is 1.44 xx 10^(-5) when partial pressure is measured in atmosphere. The corresponding value of Kc with concentration in mol//L is: