A 0.287-g sample of bianthracene (C28H18) is burned in a bomb calorimeter and the temperature increases from 25.30 °C to 27.50 °C. The calorimeter contains 1.03E3 g of water and the bomb has a heat capacity of 856 J/°C. Based on this experiment, calculate ΔE for the combustion reaction per mole of bianthracene burned (kJ/mol).
heat released by the combusiton of 0.287 g of bianthracene = heat gained by water
= mass of water * T * Cp of water
given mass of water = 1.03 * 103 g = 1030 g
Cp of water = 4 J/g.C
T = 27.5 - 25.3 = 2.2 C
heat gained by water = 1030 g * 4 J/g.C * 2.2 C = 9064 J
heat gained by bomb = 856 J/C * (27.5 - 25.3) C = 1883.2 J
Total heat change = 9064 J + 1883.2 J = 10947.2 J = 10.95 kJ
Mass of bianthracene = 0.287 g
Molar mass of bianthracene = 354 g/mol
No. of moles of bianthracene = 0.287 g/ 354 g/mol = 8.11 * 10-4 moles
E = 10.95 kJ / 8.11 * 10-4 moles = 13506.3 kJ/mol Answer
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