Camphor has a heat of combustion of5903.6 a sample of comfort having mass of 0.1204 gram is burn in a bond calorimetry the temperature increase by 2.28 degree centigrade calculate the heat capacity of the calorimetre
First, we need to calculate the amount of heat produced by burning the camphor sample:
Q = m * ΔT * C
Where Q is the heat produced, m is the mass of camphor burned, ΔT is the temperature change of the calorimeter, and C is the heat capacity of the calorimeter.
m = 0.1204 g
ΔT = 2.28°C = 2.28 K
Q = 5903.6 J/g
So, Q = 0.1204 g * 2.28 K * C
Solving for C, we get:
C = Q / (m * ΔT) = 5903.6 J/g / (0.1204 g * 2.28 K)
C = 2071.5 J/K
Therefore, the heat capacity of the calorimeter is approximately 2071.5 J/K.
To calculate the heat capacity of the calorimeter, we can use the formula:
Heat capacity = (Heat released or absorbed) / (Temperature change)
Step 1: Convert the mass of the comfort sample from grams to moles.
The molar mass of camphor (C10H16O) is approximately 152.23 g/mol.
Number of moles = mass / molar mass = 0.1204 g / 152.23 g/mol = 0.0007906 mol
Step 2: Calculate the heat released or absorbed by the combustion of camphor.
Heat released = Heat of combustion × number of moles
Heat released = 5903.6 J/g × 0.0007906 mol = 4.667 J
Step 3: Calculate the heat capacity of the calorimeter using the formula mentioned earlier.
Heat capacity = Heat released / Temperature change
Heat capacity = 4.667 J / 2.28 °C = 2.045 J/°C
Therefore, the heat capacity of the calorimeter is 2.045 J/°C.