posted by Sean on .
When 22.7mL of o.500 M H2SO4 is added to 22.7mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50 degrees Celsius, the temperature rises to 30.17 degrees Celsius. Calculate the delta h of this reaction. (Assume that the total volume is the sum of individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g x degrees Celsius.)
H2SO4 + 2KOH ==> 2H2O + K2SO4
millimoles H2SO4 = mL x M = 22.8 x 0.5 = approximately 11 (but that's an estimate).
millimoles KOH = 22.7 x 1.00 M = 22.7 mmols KOH.
q = delta H = mass H2O x specific heat x (Tfinal-Tinitial)
volume = 22.7 + 22.7 = 45.4 mL; use density to convert to grams.
q = grams x specific heat x delta T.
That gives you dH for the reaction.