Ba(OH)2 + 2HCl ==> BaCl2 + 2H2O
mols Ba(OH)2 = M x L = 0.0186
mols HCl = M x L = 0.0372
These neutralize each other exactly and will produce 0.0372 mol H2O
q = mass H2O x specific heat H2O x delta T
q = 120 g x 4.184 J/g*C x (26.41-22.19)
q = approx 2000 J but you need to redo that more accurately.
Then q = dH rxn. Technically the problem only asks for dH for the reaction and that is approx 2 kJ. However, my experience tells me the problem REALLY want kJ/mol so
approx 2 kJ/0.0372 mol = approx ? kJ/mol
In a constant-pressure calorimeter, 60.0 mL of 0.310 M Ba(OH)2 was added to 60.0 mL of 0.620 M HCl. The reaction caused the temperature of the solution to rise from 22.19 °C to 26.41 °C. If the solution has the same density and specific heat as water, what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.
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