100 ml `0.5 M H_(2)SO_(4)` (strong Acid) is neutralised by 200 ml 0.2 M `NH_(4)OH` . In a constant pressure calorimeter which results in temperature rise of `1.4 ^(@) C ` . If heat capacity of calorimeter constant is `1.5 kJ// ^(@) C` .
Which statement is /are correct .
Given `HCl + NaOH to NaCl + H_(2)O + 57 kJ CH_(3) COOH + NH_(4) OH to CH_(3) COO NH_(4) + H_(2) O + 48.1 kJ`
Ethalpy of neutralisation of HCl v/s `NH_(4) OH` is `-52.5` kJ/mol

Explanation

Total heat evolved due to the neutralization
`= C xx Delta t = 1.5 xx 1.4 = 2.1`
M.eg of `H_(2)SO_(4) = 100 xx 0.5 = 50`
M.eq of `NH_(4)OH = 20 xx 0.2 = 40`
Since `NH_(4)OH` is limiting hence energy will evolved according to it .
`implies 0.04` gm eq produces 2.1 kJ
1 gm eq produces = `(2.1)/(0.04) xx 1 = (210)/(4) = 52.5`
`implies ` Heat of neutralisation = `-52.5 kJ`