If the solution has the same density and specific heat as water, what is ΔH for this reaction (per mole of H2O produced)?

Question

In a constant-pressure calorimeter, 65.0 mL of 0.330 M Ba(OH)2 was added to 65.0 mL of 0.660 M HCl.

The reaction caused the temperature of the solution to rise from 23.77 °C to 28.27 °C.

If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g·°C, respectively), what is ΔH for this reaction (per mole of H2O produced)?
 
Assume that the total volume is the sum of the individual volumes.

Roger the Mole · Accepted Answer

Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O

The reactants are present in their stoichiometric ratio, so there is no excess and either could be considered the limiting reactant.

(65.0 mL + 65.0 mL) x (1.00 g/mL) = 130 g solution

(4.184 J/g·°C) x (130 g) x (28.27 °C - 23.77 °C) = 2447.64 J produced

(0.0650 L) x (0.660 mol/L HCl) x (2 mol H2O / 2 mol HCl) = 0.0429 mol H2O

(2447.64 J) / (0.0429 mol H2O) = 57055 J/mol H2O = 57.1 kJ/mol H2O

If the solution has the same density and specific heat as water, what is ΔH for this reaction (per mole of H2O produced)?

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