The equilibrium constant of a reaction doubles on increasing the temperature of the reaction from `25^(@)C to 35^(@)C.` Calculate enthalpy change of the reaction, assumpting it to be constant in this temperature range.

Explanation

` log. (K_(P))_(2)/(K_(p))_(1) = (DeltaH^(@))/(2*303 R) ( (T_(2)-T_(1))/(T_(1)T_(2)))`
Putting ` (K_(p))_(2)//((K_(p))_(1)= 2 , T_(1) = 25^(@) C = 298 K , T_(2) = 35^(@) C = 308 K , R = 8* 314 "JK"^(-1) "mol"^(-1) , "we get " `
` log 2 = (DeltaH^(@))/(2* 303 xx 8*314 "JK^(-1) "mol"^(-1)) xx ((308 - 298)K)/(298 K 308K)`
or ` Delta H^(@) = 52898 " J mol"^(-1) = 52* 898 "kJ mol"^(-1)`