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The equilibrium constant K(p), for the r...

The equilibrium constant `K_(p)`, for the reaction `N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)` is `1.6xx10^(-4)` at `400^(@)C`. What will be the equilibrium constant at `500^(@)C` if the heat of reaction in this temperature range is `-25.14` kcal?

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Verified by Experts

The correct Answer is:
A, B, D
vant Hoff equation for variation of `K_(p)` with temperature can be written as
`2.303 "log" K_(P_(2))/K_(P_(1))=(DeltaH[T_(2)-T_(1)])/(RxxT_(2)T_(1))`
`K_(P_(1))=1.6xx10^(-4), T_(1)=673 K`
`K_(P_(2))=?, T_(2)=773 K`
`DeltaH=-25.14xx10^(3) cal`
`R=2 cal`
`:. 2.303 "log" K_(P_(2))/(1.6xx10^(-4))=(-25.14xx10^(3))/(2)[(773-673)/(773xx673)]`
`K_(P_(2))=1.462xx10^(-5) "atm"^(-2)`
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