A 2.25 g sample of hydrazine, N2H4, is burned in a bomb calorimeter that contains 6,402.45 g of H2O, and the temperature increases from 25.00° C to 26.17° C. The heat capacity of the calorimeter is 3.64 kJ/° C. Calculate Delta E for the combustion of N2H4 in kJ/g.

Answer 1

25-26.16 = -1.17

q1=(6402.45 * 4.184 * -1.17)/1000=-A KJ

q2 = 3.64 * -1.17 = -B KJ

Delta_E = (q1 + q2)/2.25 = - C KJ/g