At constant volume the heat of combustion of a particular compound is -3378.0 kj/mol.When 1.563 g of this compound ( molar mass of 126.88 g/mol )was burned temp rose 6.991 C. What's the heat capacity of the calorimeter(calorimeter is constant)?
At constant volume the heat of combustion of a particular compound is -3378.0 kj/mol.When 1.563 g of this compound ( molar mass of 126.88 g/mol )was burned temp rose 6.991 C. What's the heat capacity of the calorimeter(calorimeter is constant)? Sorry the answer needs to be in Cal/g
kj/C not cal/g that's another question I'm working on
Jeatcombustion*moles=heatcapacity*tempchange
solve for heat capacity.
To calculate the heat capacity of the calorimeter, we need to use the equation:
q = mcΔT
Where:
q = heat transferred to or from the system
m = mass of the substance being heated or cooled
c = specific heat capacity of the substance
ΔT = change in temperature
In this case, the compound is burned in the calorimeter, and the heat transferred to the system is the heat of combustion.
Given:
Heat of combustion (q) = -3378.0 kJ/mol
Mass of compound (m) = 1.563 g
Molar mass of compound (M) = 126.88 g/mol
Temperature change (ΔT) = 6.991 °C
First, we need to calculate the number of moles of the compound burned:
n = m/M
n = 1.563 g / 126.88 g/mol
Next, we need to convert the heat of combustion from kJ/mol to J/mol:
q = -3378.0 kJ/mol × (1000 J/1 kJ)
Now, we can calculate the heat capacity of the calorimeter:
q = mcΔT
Since the calorimeter is constant, its heat capacity is equal to the negative of the heat transferred to the system. Therefore:
q = -CΔT
Where C is the heat capacity of the calorimeter.
Rearranging the equation, we have:
C = -q/ΔT
So, we can substitute the values into the formula to find the heat capacity:
C = (-3378.0 × 1000)/(6.991 °C)
Finally, we can calculate the heat capacity by performing the calculation:
C = -4833558/6.991
C ≈ -691409 J/°C
Therefore, the heat capacity of the calorimeter is approximately -691409 J/°C.