Asked by ny
A sample of ethanol (C2H6O) has a mass of 0.2301 g. Complete combustion of this sample causes the temperature of a bomb calorimeter to increase by 1.33°C. The calorimeter has a mass of 2.000 kg and a specific heat of 2.45 J/g•°C.
What is the heat of combustion for this sample?
kJ
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q = m c ΔT = (2000 g)(2.45 J/g·°C)(1.33 °C) = 6517 J = 6.52 kJ.
The reaction is exothermic, so q = -6.52 kJ for the sample.
Per mole of C2H6O: n = 0.2301 g / 46.07 g·mol−1 = 0.004996 mol, so ΔHcomb ≈ -1305 kJ·mol−1.
The reaction is exothermic, so q = -6.52 kJ for the sample.
Per mole of C2H6O: n = 0.2301 g / 46.07 g·mol−1 = 0.004996 mol, so ΔHcomb ≈ -1305 kJ·mol−1.
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