text: rocket science? hydrazine, n2h4 , and its derivatives are widely used as rocket fuels. the combustion of hydrazine with oxygen produces n2 (g) and h2o (g). when 1.90 grams of hydrazine is burned in a bomb calorimeter, the temperature of the calorimeter rises by 4.20oc. the calorimeter contains 925.0 g of water, and the bomb has a heat capacity of 887.0 j/k. what is the heat of reaction in kj/mol for the combustion of one mole of hydrazine? i searched through my thermodynamics book for this, so i hope you appreciate it. first, you need a ballanced chemical equation.  2n2h2 + o2 ---> 2h2o + 2n2  c = 887.0 j/k = 0.8870 kj/ k n = 1 mol (since it's a 2 to 2 relation, we can just say 1) delta t = t = 4.20 ºc = 4.20 k q = ?  q = ct/n = (0.8870 kj/k * 4.20 k) / (1 mol)    =  3.73 kj/mol   hope this helps!