A hydrocarbon sample was burned in a bomb calorimeter. The temperature of the calorimeter and the 1.00 kg of water rose from 20.45 °C to 23.65 °C. The heat capacity of the calorimeter, excluding the water, is 2.21 kJ/°C. Using this information, determine the heat released by the combustion.

heat released to raise T of water + heat to raise T of calorimeter = total heat released.

[mass water x specific heat water x delta T] + [2210 J/C x delta t] = q
Check my thinking.

To determine the heat released by the combustion, we can use the equation:

q = mcΔT

where q is the heat released (in joules), m is the mass of the water (in kg), c is the specific heat capacity of water (4.18 J/g°C or 4180 J/kg°C), and ΔT is the change in temperature (in °C).

First, let's calculate the mass of the water:

m = 1.00 kg

Next, let's calculate ΔT:

ΔT = (23.65 °C - 20.45 °C) = 3.20 °C

Now, let's calculate the heat released:

q = mcΔT

q = (1.00 kg) × (4180 J/kg°C) × (3.20 °C)

q ≈ 13,376 J

However, in this specific problem, we have the heat capacity of the calorimeter excluding the water instead of the specific heat capacity of water. So, we need to take into account the heat absorbed by the calorimeter.

Let's calculate the heat absorbed by the calorimeter:

q_calorimeter = CΔT

where q_calorimeter is the heat absorbed by the calorimeter (in joules), C is the heat capacity of the calorimeter (2.21 kJ/°C or 2210 J/°C), and ΔT is the change in temperature (in °C).

ΔT = 3.20 °C

q_calorimeter = (2.21 kJ/°C) × (3.20 °C) × (1000 J/kJ)

q_calorimeter = 22,464 J

The heat released by the combustion is equal to the heat absorbed by the calorimeter:

q = q_calorimeter

q = 22,464 J

Therefore, the heat released by the combustion is approximately 22,464 J.