Question

a 4.18 g sample of a hydrocarbon is combusted in a bomb calorimeter that contains 974 g of water. the temperature of the water increases by 6.9 oc when the hydrocarbon is combusted. the calorimeter constant for the calorimeter was determined to be 624 j/oc. what is the heat of the reaction, in kj, when 4.18 g of the hydrocarbon are combusted? ch2o(l)

Answer 1

The heat of the reaction, in kJ, when 4.18 g of the hydrocarbon are combusted 775.70 kJ.

The heat energy is given as :

q = m c ΔT + Ccal ΔT

q = ( 974 g× 4.184 ×6.9) + 624 ×6.9

q = 32424.59 J

moles of hydrocarbon = 0.0418 mol

heat of combustion = 32424.59 J / 0.0418 mol

                                 = 775707.89 J

                                = 775.70 kJ

Thus, A 4.18 g sample of a hydrocarbon is combusted in a bomb calorimeter that contains 974 g of water. the temperature of the water increases by 6.9 °C when the hydrocarbon is combusted. the calorimeter constant for the calorimeter was determined to be 624 J/°C. what is the heat of the reaction is 775.70 kJ.

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