the equillibrium constant `K_(P)` for the reaction , `N_(2)(g)+ 3H_(2)(g)Leftrightarrow2NH_(3)(g)` `1.6 xx 10^(-4) (atm)^(-2) at 400^(@)C` if heat of the reaction in this temoerture range is -25.14 kcal ?A. ` 1.231 xx 10^(-4)(atm)^(-2)`B. `1.876 xx 10^(-7)(atm)^(-2)`C. `1.462 xx 10^(-5)(atm)^(-2)`D. `3.462 xx 10^(-5)(atm)^(-2)`

the equillibrium constant `K_(P)` for the reaction , `N_(2)(g)+ 3H_(2)

1.	the equillibrium constant `K_(P)` for the reaction , `N_(2)(g)+ 3H_(2)(g)Leftrightarrow2NH_(3)(g)` `1.6 xx 10^(-4) (atm)^(-2) at 400^(@)C` if heat of the reaction in this temoerture range is -25.14 kcal ?A. ` 1.231 xx 10^(-4)(atm)^(-2)`B. `1.876 xx 10^(-7)(atm)^(-2)`C. `1.462 xx 10^(-5)(atm)^(-2)`D. `3.462 xx 10^(-5)(atm)^(-2)`
Answer» Correct Answer - c Equilibrium constants at different temperature and heat of the reaction are related by the equation `2.303 log(K_(P_(2))/(K_(p_(1))))= (DeltaH^(@))/R[(T_(2)-T_(1))/(T_(1)T_(2))]` `log K_(P_(2))=-4.835` `K_(P_(2))=1.462xx10^(5)(atm)^(-2)`

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