Under constant-volume conditions the heat of combustion of glucose is 15.57 kJ/g. A 2.500g sample of glucose is burned in a bomb calorimeter. The temperature of the calorimeter increses from 20.55 C to 23.25 C. What is the total heat capacity of the calorimeter?

Which equations would you use to solve this problem?

q = C*delta T

You know q = 15.57 kJ/g and you know you start with 2.5 g. You know delta T.

Well, to solve this problem, there are a couple of equations you can use. You'll need to use the equation for calculating heat transfer, as well as the equation for calculating heat capacity. So grab your calculators and let's get started!

To solve this problem, we can use the equation:

q = C * ΔT

where:
- q is the heat transferred to the calorimeter
- C is the heat capacity of the calorimeter
- ΔT is the change in temperature

With the given data, we can rearrange the equation to solve for C:

C = q / ΔT

Let's substitute the known values into the equation and solve for C.

To solve this problem, you need to use the equation for heat capacity (C):

C = q / ΔT

Where C is the heat capacity, q is the heat transferred, and ΔT is the change in temperature.

In this case, you are given the mass (2.500g) and the heat of combustion of glucose (15.57 kJ/g). To calculate the heat transferred (q), you can use the equation:

q = m * ΔH

Where q is the heat transferred, m is the mass of the substance burned (2.500g), and ΔH is the heat of combustion of glucose (15.57 kJ/g).

Once you have calculated the heat transferred (q), you can then calculate the total heat capacity (C) of the calorimeter using the equation mentioned earlier:

C = q / ΔT

Where C is the total heat capacity, q is the heat transferred, and ΔT is the change in temperature (23.25 °C - 20.55 °C).