Answer to Question #168377 in General Chemistry for Dawson

Question

I am pretty sure I did this completely wrong. When 25.8 mL of 0.500 M H2SO4 is added to 25.8 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH...

of this reaction. (Assume that the total volume is the sum of the 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·°C.) Do not answer in scientific notation. 

I got -0.0558 kJ/mol H2O which is wrong.

Answer 1

$ΔH= m×c×dT$

dT= 30.17- 23.50= 6.67⁰C

Total volume=25.8+ 25.8=51.6ml

Density = mass/volume

Mass=51.6g

ΔH=51.6 ×4.184× 6.67=1440.02 J/g.⁰C