Ba(OH)2 + 2HCl ==> 2H2O + BaCl2
mols Ba(OH)2 = M x L = ?
mols HCl = M x L = ? which is twice that of Ba(OH)2 so the two exactly neutralize each other.
q = heat generated = mass H2O x specific heat H2O x (Tfinal-Tinitial)
mass H2O = 65 + 65 = 130 mL = 130 g
specific heat H2O = 4.184 J/g*C
Tfinal given
Tinitial given
solve for q = delta H for the reaction.
delta H per mols H2O is delta H rxn/mols H2O produced
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 24.28 °C to 28.78 °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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