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The values of K(p)//K(c) for the followi...

The values of `K_(p)//K_(c)` for the following reactions at 300 K are, respectively :
(At 300 K, RT = 24.62 d`m^(3)` atm `mol^(-1)`)
`N_(2)(g)+O_(2)(g)hArr 2 NO(g)`
`N_(2)O_(4)(g)hArr2 NO_(2)(g)`

A

`"1,24.62 dm"^3 "atm mol"^(-1) , 606.0 dm^6 atm^2 mol^(-2)`

B

`1,4.1xx10^(-2) dm^(-3) atm^(-1) mol^(-1) , 606.0 dm^6 atm^2 mol^(-2)`

C

`1,606.0 dm^6 atm^2 mol^(-2), 1.65xx10^(-3) dm^3 atm^(-2) mol^(-1)`

D

`1,24.62 dm^3 atm mol^(-1) , 1.65xx10^(-3) dm^(-6) atm^(-2) mol^2`

Text Solution

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The correct Answer is:
D
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K_(p)//K_(c) for the reaction CO(g)+1/2 O_(2)(g) hArr CO_(2)(g) is

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Equilibrium constant K_(C) for the following reaction at 800 K is, 4 NH_(3)(g)hArr (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g) . The value of K_(p) for the following reaction will be N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)

The equilibrium constant for the following reactions at 1400 K are given. 2H_(2)O(g)hArr2H_(2)(g) + O_(2)(g) , K_(1)=2.1×x10^(-13) 2CO_(2)(g) hArr2CO(g)+O_(2)(g),K_(2) = 1.4 x× 10^(-12) Then, the equilibrium constant K for the reaction H_(2)(g) + CO_(2)(g)hArrCO(g) + H_(2)O(g) is

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