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:

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{-}}{{\mathbf{C}}}_{{\mathbf{cal}}}{\mathbf{\u2206}}{\mathbf{T}}}$

q = heat

C_{cal }= heat capacity of the calorimeter

ΔT = T_{f} – T_{i}

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

Under constant-volume conditions the heat of combustion of glucose (C_{6}H_{12}O_{6}) 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 ^{o}C to 24.75 ^{o}C.

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

Frequently Asked Questions

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.

What professor is this problem relevant for?

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