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 celsius to 23.65 celsius.The heat capacity of the caloimeter, excluding the water, is 2.21 kJ/degree celsius. using this information, determine the heat released by the combustion.
I have no idea how to do this. Please explain steps so I can see how to do it for myself
The heat released is the total of the heat required to raise the temperature of the water (1,000 grams) + heat to raise the temperature of the calorimeter.
q = [mass H2O x specific heat water x (Tfinal-Tinitial)] + [cal x (Tfinal-Tinitial)]] = 0
Solve for q.
a 151g quantity of water at 30.0 celsius was heated to boiling and 35.0 g of that water was converted to steam. what is the heat input required in calories to do this?
To determine the heat released by the combustion, we will use the equation:
q = m * C * ΔT
where:
q = heat released
m = mass of water (in kg)
C = specific heat capacity of water (4.18 J/g°C or 4186 J/kg°C)
ΔT = change in temperature (in °C)
Step 1: Convert the heat capacity of the calorimeter to joules.
Given:
Heat capacity of calorimeter = 2.21 kJ/°C
To convert this to joules, multiply it by 1000 (since 1 kJ = 1000 J).
2.21 kJ * 1000 = 2210 J/°C
Step 2: Calculate the change in temperature of the water.
Given:
Initial temperature = 20.45 °C
Final temperature = 23.65 °C
ΔT = Final temperature - Initial temperature
ΔT = 23.65 °C - 20.45 °C = 3.20 °C
Step 3: Calculate the heat released by the combustion.
Given:
Mass of water = 1.00 kg
Specific heat capacity of water = 4186 J/kg°C
Using the equation q = m * C * ΔT, plug in the values:
q = (1.00 kg) * (4186 J/kg°C) * (3.20 °C)
q = 1.00 kg * 4186 J/kg°C * 3.20 °C
q = 13354.88 J
Step 4: Calculate the total heat released, including the calorimeter.
The heat released only accounts for the water. Since the calorimeter also absorbs heat, we need to calculate the heat absorbed by the calorimeter separately.
Given:
Heat capacity of calorimeter = 2210 J/°C
Using the equation q = m * C * ΔT:
q_calorimeter = (1.00 kg) * (2210 J/°C) * (3.20 °C)
q_calorimeter = 7104 J
To find the total heat released, we add the heat released by the water and the heat released by the calorimeter:
Total heat released = heat released by water + heat released by calorimeter
Total heat released = 13354.88 J + 7104 J
Total heat released = 20458.88 J
Therefore, the heat released by the combustion is 20458.88 J.
To determine the heat released by combustion, you can use the concept of calorimetry. Calorimetry is the process of measuring the heat exchanged during a chemical or physical process.
Here are the steps you can take to solve this problem:
1. Calculate the change in temperature (∆T) of the water in the calorimeter.
∆T = Final temperature - Initial temperature
∆T = 23.65°C - 20.45°C
2. Convert the mass of water from grams to kilograms:
Mass of water = 1.00 kg
3. Calculate the heat absorbed by the water using the specific heat capacity of water.
Heat absorbed by water = (Mass of water) * (Specific heat capacity of water) * (∆T)
The specific heat capacity of water is approximately 4.18 J/(g·°C).
4. Calculate the heat capacity of the calorimeter (excluding water).
Heat capacity of calorimeter = 2.21 kJ/°C
5. Calculate the total heat absorbed by both the water and the calorimeter.
Total heat absorbed = Heat absorbed by water + Heat capacity of calorimeter
6. The total heat absorbed is equal to the heat released by combustion.
Heat released by combustion = Total heat absorbed
By following these steps, you can find the heat released by the combustion process. Remember to convert all units as necessary and keep track of the units to ensure they cancel out and yield the correct final unit for heat.