A constant pressure calorimeter consists of an insulated neaker of mass `92g` made up of glass with heat capacity `0.75 J K^(-1) g^(-1)`. The beaker contains `100 mL` of `1M HCI` at `22.6^(@)C` to which `100 mL` of `1M NaOH` at `23.4^(@)C` is added. The final temperature after the reactions is complete is `29.3^(@)C`, What is `DeltaH` per mole for this neutralization reaction? Assume that the heat capacities of all solutions are equal that of same volumes of water.

Explanation

Initial average temperature of the acid and base
`=(22.6 +23.4)/(2) = 23.0^(@)C`
Rise is temperature `=(293.-23.0) = 6.3^(@)C`
Total heat produced `= mC DeltaT`
`(92 xx 0.75 + 200 xx 4.184) xx 6.3`
`=(905.8) xx 6.3 = 5706.54 J`
Ethalpy of neutralisation `=- (5706.54)/(100) xx 1000 xx1 =- 57065.4 J =- 57 kJ`