Following data is given for the reaction : CaCO_(3) (s) rarr CaO(s) + CO_(2) (g) Delta_(f) H^( Θ) [CaO(s) ] = - 635.1 kJ "mol" ^(-1) Delta_(f) H^(Θ) [ CO_(2) (g) ] = - 393.5 kJ"mol" ^(-1) Delta_(f) H^(Θ)[CaCO_(3)(s) ] = - 1206.9 kJ "mol" ^(-1) Predict the effect of temperature on the equilibrium constant of the above reaction.

Following data is given for the reaction : CaCO_(3) (s) rarr CaO(s) +

1.	Following data is given for the reaction : CaCO_(3) (s) rarr CaO(s) + CO_(2) (g) Delta_(f) H^( Θ) [CaO(s) ] = - 635.1 kJ "mol" ^(-1) Delta_(f) H^(Θ) [ CO_(2) (g) ] = - 393.5 kJ"mol" ^(-1) Delta_(f) H^(Θ)[CaCO_(3)(s) ] = - 1206.9 kJ "mol" ^(-1) Predict the effect of temperature on the equilibrium constant of the above reaction.
Answer» SOLUTION :`delta_(r) H^(@) = Delta_(f) H^(@) [CaO (s) ] + Delta_(f) H^(@)[CO_(2)(g) ] -Delta_(f) H^(@)[CaCO_(3)(s)]` `=- 635.1 + (-393.5) - (-1206.9) = 178.3 kJ"mol"^(-1)` Thus, the reaction is endothermic. Hence, according to Le Chatelier'sprinciple, onincreasingthe temperature, the equilibrium will PROCEED in the FORWARD direction .