50.0 mL of 1.00 M HCl solution are mixed with 30.0 mL of 2.00 M NaOH solution in a coffee-cup
calorimeter. The initial temperature of the solutions before mixing is 20.5 C. The highest
temperature recorded after mixing is 29.8 C. The total mass of the solution is 80.5 g. Calculate
a) the heat change, q, in joules, accompanying this reaction and state whether the process is exo- or
endothermic b) the enthalpy of neutralization, ∆H , in kJ/mol. ( swater = 4.184 J/g C )
[ a) q = – 3,132.35 = –3.1 x 103 J = –3.1 kJ, exothermic process b) ∆H = – 63 kJ/mol ]
I get a) but how do I find b)?
Any help would be greatly appreciated!
Thanks in advance!