Question

Enter your answer in the provided box.

When 22.9 mL of 0.500 M H₂SO₄ is added to 22.9 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.)

_______kJ/mol H₂O

Answer 1

Balance reaction is---

H2SO4 + 2KOH --> K2SO4 + 2H2O

Moles of H2O = Moles of KOH ( from balanced reaction)

= 1.00*0.0229 = 0.0229 moles

Total volume = 22.9 + 22.9 = 45.8 ml

Mass of solution = 1.00*45.8 = 45.8 gram

Heat absorb by solution = mcdT

= 45.8*4.184*(30.17-23.50)

= 1278.153424 J

dH of the reaction = -heat absorb by solution/moles oh H2O

= -1278.153424/0.0229

= -55814.56 J/mol H2O

= -55.8 kJ/mol H2O

If you have any query please comment

If you satisfied with the solution please rate it thanks