Problem: Find ΔH for the combustion of ethanol (C2H6O) to carbon dioxide and liquid water from the following data. The heat capacity of the bomb calorimeter is 34.65 kJ/K and the combustion of 1.761 g of ethanol raises the temperature of the calorimeter from 294.26 K to 295.77 K .

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Step 1

q = CcalTq = (34.65kJK)(295.77 K - 294.26 K)

q = 52.3215 kJ


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Problem Details

Find ΔH for the combustion of ethanol (C2H6O) to carbon dioxide and liquid water from the following data. The heat capacity of the bomb calorimeter is 34.65 kJ/K and the combustion of 1.761 g of ethanol raises the temperature of the calorimeter from 294.26 K to 295.77 K .

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Constant-Volume Calorimetry concept. You can view video lessons to learn Constant-Volume Calorimetry. Or if you need more Constant-Volume Calorimetry practice, you can also practice Constant-Volume Calorimetry practice problems.

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Based on our data, we think this problem is relevant for Professor Morkowchuk's class at UVA.