Question

When 23.6 g of calcium chloride, CaCl2, was dissolved in water in a constant-pressure calorimeter, the temperature rose from 25.0 C to 38.7 C. If the heat capacity of the solution and the calorimeter is 1258 J/C, what is the enthalpy change when 0.710 mol of calcium chloride dissolves in water? The solution process is CaCl2(s) --> Ca2+(aq) + 2Cl–(aq)

Answer 1

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dus) concept 222222222 Heat realoved in Ron = Heat gain to ride the temp. Steh o find Heat required to sail Tem. fuam 25" to 38.7°C AT= 38.7-25 = 13.5°C C = 12585/6 Heat =COT Heat = 1258 T/CX 13.5°C Heat = 16983] = Heat realsed in Ron 6. Enthalpy change = - Heat realed in Ron = -16983J Stehlü find Enthalpy Chonge here mole of cacle. Ca Cly (5) - Ca2f109) +261 (ar) Sho = Enthalpy change - 169835 x 1KJ males of calls - 7236g 1035 110.9 g/mol sn= -79.8 KJ /mal (o'moles = mass I find Enthalpy change for 0 • Ilmol Calda Sl= moles X AHO ZH = 0. Ilmal x 79.8 kJ/mol A = -56-66 KJ du aumas