a) We will calculate amount of heat using:
Q = Cp · m · ΔT,
where Ср – the specific heat, J/(g·K);
m – mass of solution;
ΔT – change of temperature, K.
Having substituted data from a statement of the problem in this formula, we will receive:
Q = 4,183·(1,0*100 +1,0*100) · (23,4 – 20,1) = 2760,78 J.
ΔН = – Q = –2760,78 J < 0 – reaction is exothermic.
b) Number of moles of sodium hydroxide equals to number of moles of HCl:
νNaOH = νHCl = 0,5*100/1000 = 0.05 mol
Then the molar enthalpy in kJ mol-1 ( Hm) for the reaction is equal:
Hm = – Q = –2760,78/0,05 = –55215,6 J/mol = –55,22 kJ/mol.
Answer: a) ΔН =–2760,78 J < 0 – reaction is exothermic;
b) Hm = –55,22 kJ/mol.
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