The relation between `K_(p)` and `K_(c)` is `K_(p)=K_(c)(RT)^(Deltan)` unit of `K_(p)=(atm)^(Deltan)`, unit of `K_(c)=(mol L^(-1))^(Deltan)`
The equilibrium constant of the following reactions at `400 K` are given:
`2H_(2)O(g) hArr 2H_(2)(g)+O_(2)(g), K_(1)=3.0xx10^(-13)`
`2CO_(2)(g) hArr 2CO(g)+O_(2)(g), K_(2)=2xx10^(-12)`
Then, the equilibrium constant K for the reaction
`H_(2)(g)+CO_(2)(g) hArr CO(g)+H_(2)O(g)`
is

Options

A. `2.58`
B. `0.066`
C. `15`
D. `0.38`

Explanation

`K_(c_(1))=2.1xx10^(-13)=([H_(2)]^(2)[O_(2)])/([H_(2)O]^(2))`
`K_(c_(2))=1.4xx10^(-12)=([CO]^(2)[O_(2)])/([CO_(2)]^(2))`
`K_(c_(3))=([H_(2)O][CO_(2)])/([H_(2)][CO])`
`=sqrt(K_(c_(1)))/(K_(c_(2)))=sqrt((1.4xx10^(-12))/(2.1xx10^(-13)))=2.58`