Question

When 27.0 mL of 0.500 M H2SO4 is added to 27.0 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.)

Answer: ______  kJ/mol H2O

Answer 1

Reaction: H₂ Soy it 2KOH K Soy + 2H₂O m.mole of H₂ Soy = 27 x 0.5 = 13.5 m.mole of koy - 27 x 27 .. teo + 2H₂O H₂ Soy + 2 kot - 13.5 27 o oooo ₂ Soy o 13.5 27 mimole more of Hoo on Ho formed formed a 27 a 27 X 103 Now Heat released a mSoT S= 4.184 3/g c for mass of solution - volume x density (27 +27) x1 = 549 .. Heat = 544.184 × (30.17 - 23.57 - 1506.99 Joule Intor & for 27 x 103 mol H₂o Heat = 150699] for Imole H₂o Heat = 1506. gg. 27 x 103 - 55,814 Joule = 55.814 kJ . In Cup Cal con meter, Heat = OH DH = -55.814 KI) mol of Had