Two solutions, initially at 24.60°c, are mixed in a coffee cup calorimeter (ccal = 15.5 j/° c. when a100.0 ml volume of 0.100 m agno3 solution is mixed with a 100.0 ml sample of 0.200 m naclsolution, the temperature in the calorimeter rises to 25.30° c. determine the ? h°rxn for thereaction as written below. assume that the density and heat capacity of the solutions is the sameas that of water. nacl (aq) + agno3(aq) ? agcl(s) + nano3(aq) ? h°rxn = ?

The solution is as follows:

Since the mass of the calorimeter is given, let's take the heat effects of the calorimeter as negligible.

Compute for sensible heat from 24.60°C (297.6 K) to 298 K. The heat capacity of water is 4.18 J/g·K.
ΔH₁ = ∫[(0.1 mol/L AgNO₃)(0.1 L)(169.87 g/mol AgNO₃)(4.18 J/g·K)dT + (0.2 mol/L NaCl)(0.1 L)(58.44 g/mol NaCl)(4.18 J/g·K)dT]
Take the integral from limits 297.6 K to 298.8 K(25.30°C).
ΔH₁ = 4,289.12 J

Compute for the heat of reaction at room temperature:
ΔH₂ = ∑(Heat of formation of products*stoichiometric coefficient) - ∑(Heat of formation of reactants*stoichiometric coefficient)
ΔH₂ = [(-127 kJ/mol AgCl)(1 mol) + (-467 kJ/mol NaNO₃)(1 mol)] - [(-123.02 kJ/mol AgNO₃)(1 mol) + (−407.27 kJ/mol NaCl)(1 mol)]
ΔH₂ = -63.71 kJ or -63,710 J

Thus,
ΔHrxn = ΔH₁ + ΔH₂ = 4,289.12 J + -63,710 J
ΔHrxn = 59,420.88 J or 59.42 kJ

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