Ba(OH)2 + 2HCl ==> BaCl2 + 2H2O
mols Ba(OH)2 = M x L = 0.320 x 0.050 = 0.016
heat released = mass H2O x specific heat H2O x (Tfinal-Tinitial)
q = 100 x 4.184 x (26.16-21.80) = ?
q/0.016 = q/2 mol H2O so divide by 2 for q/1 mol H2O produced and add a negative sign since heat is released. Divide by 1000 to convert to kJ/mol H2O produced. The answer should be about 57 kJ/mol
In a constant-pressure calorimeter, 50.0 mL of 0.320 M Ba(OH)2 was added to 50.0 mL of 0.640 M HCl. The reaction caused the temperature of the solution to rise from 21.80 °C to 26.16 °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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