When 0.1523 g of liquid pentane (c_5 5 h_{12} 12 ) combusts in a bomb calorimeter, the temperature rises from 23.7^{\circ} ∘ c to 29.8 ^{\circ} ∘
c. what is \deltaδu_{rxn} rxn for the reaction in kj/mol pentane? the heat capacity of the bomb calorimeter is 5.23 kj/^{\circ} ∘
c?
q solution = m x c x ΔT
m solution = 0.468 g pentane + 1,000 g H2O
= 1,000.468 g solution
c solution = c water = 4.184 J/g.°C
ΔT = Tf - Ti = 23.65 °C - 20.45 °C = 3.20 °C
q solution = 1,000.468 g x 4.184 J/g.°C x 3.20 °C
= 13.395 kJ
