Constant-Volume Calorimetry Video Lessons

Concept: Heat of Combustion

# Problem: Under constant-volume conditions the heat of combustion of glucose (C6H12O6) is 15.57 kJ/g. A 3.550 -g sample of glucose is burned in a bomb calorimeter. The temperature of the calorimeter increased from 20.95 oC to 24.75 oC.If the size of the glucose sample had been exactly twice as large, what would the temperature change of the calorimeter have been?

###### FREE Expert Solution

We’re being asked to determine the temperature change if the size of the glucose sample had been exactly twice as large.

We will use the heat of combustion of glucose to calculate the temperature change. Recall that heat can be calculated using the following equation:

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{-}}{{\mathbf{C}}}_{{\mathbf{cal}}}{\mathbf{∆}}{\mathbf{T}}}$

q = heat
Ccal = heat capacity of the calorimeter
ΔT = Tf – Ti

We will do the following steps to solve the problem:

Step 1: Calculate the specific heat capacity of the calorimeter

Step 2: Calculate the temperature change

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###### Problem Details

Under constant-volume conditions the heat of combustion of glucose (C6H12O6) is 15.57 kJ/g. A 3.550 -g sample of glucose is burned in a bomb calorimeter. The temperature of the calorimeter increased from 20.95 oC to 24.75 oC.

If the size of the glucose sample had been exactly twice as large, what would the temperature change of the calorimeter have been?