Problem: The combustion of 1 mole of glucose C6H12O6 releases 2.82×103 kJ of heat. If 1.25 g of glucose are burnt in a calorimeter containing 0.95 kg of water and the temperature of the entire system raises from 20.10 °C to 23.25 °C. What is the heat capacity of the calorimeter?

FREE Expert Solution

We’re being asked to calculate the heat capacity of the calorimeter. This is given by the equation:

qrxn=qcalorimeter+qsolution

where qcalorimeter = heat absorbed by the calorimeter and qsolution = heat absorbed by the water in the calorimeter. 


Expanding this, we have:

qrxn=CcalT+mcT

where 

Ccal = heat capacity of the calorimeter
m = mass of water (in grams)
c = specific heat capacity of water
ΔT = change in temperature = final T – initial T.

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Problem Details

The combustion of 1 mole of glucose C6H12O6 releases 2.82×103 kJ of heat. If 1.25 g of glucose are burnt in a calorimeter containing 0.95 kg of water and the temperature of the entire system raises from 20.10 °C to 23.25 °C. What is the heat capacity of the calorimeter?

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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.