For the reaction `N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g)` at 298K, enthalpy and entropy changes are -92.4 kJ and -198.2 `JK^(-1)` respectively. Calculate the equilibrium constant of the reaction `(R=8.314JK^(-1)mol^(-1))`.

For the reaction `N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g)` at 298K, enthalpy

1.	For the reaction `N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g)` at 298K, enthalpy and entropy changes are -92.4 kJ and -198.2 `JK^(-1)` respectively. Calculate the equilibrium constant of the reaction `(R=8.314JK^(-1)mol^(-1))`.
Answer» Correct Answer - `6.958xx10^(5)` `DeltaG=DeltaH-TDeltaS`. Calculate `DeltaG`.

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For the reaction `N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g)` at 298K, enthalpy and entropy changes are -92.4 kJ and -198.2 `JK^(-1)` respectively. Calculate the equilibrium constant of the reaction `(R=8.314JK^(-1)mol^(-1))`.

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