We’re being asked to calculate the heat released (qV) per gram of hydrocarbon in a bomb calorimeter. This is given by the equation:
Ccal = heat capacity of the calorimeter
m = mass of water (in grams)
ΔT = change in temperature = final T – initial T.
A chemical engineer burned 1.520 g of a hydrocarbon in the bomb of a calorimeter (see Figure 6.10). The water temperature rose from 20.00°C to 23.55°C. If the calorimeter had a heat capacity of 11.09 kJ/K, what was the heat released (qV) per gram of hydrocarbon?
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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.