Camphor (C10H16O) has a heat of combustion of 5903.6 kJ/mol. When a sample of camphor with a mass of 0.124 g is burned in a bomb calorimeter, the temperature increases by 2.28 oC. Calculate the heat capacity of the calorimeter.

heat generated by camphor is

5903.6 kJ/mol x 0.124/152.24 = ? kJ
?kJ = Ccal x delta T.
Solve for Ccal.

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Well, if camphor makes the temperature rise, it sounds like it's quite hot stuff! Let's calculate the heat capacity of the calorimeter to see just how hot it can get.

First, we need to convert the mass of camphor from grams to moles. To do that, we divide the mass (0.124 g) by the molar mass of camphor, which is 152.23 g/mol. This gives us:
0.124 g / 152.23 g/mol = 0.000814 mol

Now, we plug in the values we have into the following formula:

q = C * ΔT

Where:
q is the heat transferred (which is equal to the heat of combustion)
C is the heat capacity of the calorimeter
ΔT is the temperature change (2.28 oC)

So, the equation becomes:

5903.6 kJ/mol = C * 2.28 oC

To convert the temperature from Celsius to Kelvin, we add 273.15 to 2.28 oC, giving us 275.43 K.

Rearranging the equation, we find:

C = 5903.6 kJ/mol / 275.43 K = 21.4 kJ/K

So, the heat capacity of the calorimeter is 21.4 kJ/K. It must be pretty good at handling all that heat from burning camphor!

To calculate the heat capacity of the calorimeter, we can use the equation:

q = C * ΔT

Where:
- q is the heat generated by the combustion of camphor
- C is the heat capacity of the calorimeter
- ΔT is the change in temperature of the calorimeter

First, let's convert the mass of camphor to moles.

Molar mass of camphor (C10H16O) = 152.23 g/mol

moles = mass / molar mass
moles = 0.124 g / 152.23 g/mol
moles = 0.000813 mol

Next, we will calculate the heat generated by the combustion of camphor.

Heat of combustion = 5903.6 kJ/mol

q = moles * heat of combustion
q = 0.000813 mol * 5903.6 kJ/mol
q = 4.79 kJ

Finally, we can plug the values into the equation to find the heat capacity of the calorimeter.

q = C * ΔT

4.79 kJ = C * 2.28 oC

To convert oC to Kelvin, we add 273.15.
ΔT = 2.28 + 273.15 = 275.43 K

C = q / ΔT
C = 4.79 kJ / 275.43 K
C ≈ 0.01739 kJ/K

Therefore, the heat capacity of the calorimeter is approximately 0.01739 kJ/K.

To calculate the heat capacity of the calorimeter, we can use the formula:

Heat capacity = Heat gained by calorimeter / Temperature change

We already have the temperature change (2.28 oC), so our next step is to determine the heat gained by the calorimeter.

To do that, we need to calculate the heat released by the combustion of camphor.

First, we need to convert the mass of camphor from grams to moles. We can use the molar mass of camphor to do this.

Molar mass of camphor (C10H16O) = (10×12.01 g/mol) + (16×1.01 g/mol) + (1×16.00 g/mol)
= 152.18 g/mol

Now, we can calculate the number of moles of camphor burned:

Number of moles of camphor = Mass of camphor / Molar mass of camphor
= 0.124 g / 152.18 g/mol
≈ 0.000814 mol

Next, we need to calculate the heat released by the combustion of camphor.

Heat released = Heat of combustion of camphor × Number of moles of camphor
= 5903.6 kJ/mol × 0.000814 mol
≈ 4.805 kJ

Now we have the heat gained by the calorimeter (4.805 kJ) and the temperature change (2.28 oC). We can calculate the heat capacity of the calorimeter.

Heat capacity = Heat gained by calorimeter / Temperature change
= 4.805 kJ / 2.28 oC
≈ 2.106 kJ/oC

Therefore, the heat capacity of the calorimeter is approximately 2.106 kJ/oC.