When 8.5 g of methane (ch4) is burned in a bomb calorimeter (heat capacity = 2.677 × 103 j/°c), the temperature rises from 24.00 to 27.08°c. how much heat is absorbed by the calorimeter? ch4(g) + 2o2(g) → co2(g) + 2h2o(l); ∆h° = –1283.8 kj?

Answer is: 8.24 kJ of heat is absorbed by the calorimeter.

ΔT= 27.08°C - 24.00°C.

ΔT = 3.08°C; temperature change of reaction.

m = 8.5 g; mass of methane.

cp= 2.677 kJ/°C, specific heat capacity of the bomb calorimeter.  

Qcal = ΔT(methane) · cp(methane).  

Qcal = 3.08°C · 2.677 kJ/°C.  

Qcal = 8.245 kJ; amount of heat absorbed.

8 carbon atoms forming single bonds with 18 hydrogen atoms; a triple bond exists between the third and fourth carbon atom from the right

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