Question

A 0.3423 g sample of pentane, C5H12, was burned in a bomb calorimeter. The temperature of the calorimeter and the 1.000kg of water contained therein rose from 20.22 degrees celcius to 22.82 degrees celcius. The heat capacity of the calorimeter is 2.21 kJ/C. The heat capacity of water = 4.184 J/g C.A. How much heat was given off during combustion fo the sample of pentane.answer = 16.6 kJB. What is the heat of combustion, in kilojoules, per gram of pentaneanswer = 48.6 kJ/g

Answer 1

`Q=16.62kJ`

Δ
`_CH=48.6kJ/g`

Step-by-step explanation:

Hello,

A. In this part, we must include the heat effect for pentane and water:

`Q=1000gH_2O*4.184J/(g^0C)*(1kJ)/(1000J) *(22.82^0C-20.22^0C)+2.21kJ/^0C*(22.82^0C-20.22^0C)\\Q=16.62kJ`

B. In this part, we just consider the previously computed heat and divide it by the sample of pentane as follows:

Δ
`_CH=(Q)/(m)=(16.6kJ)/(0.3423g)= 48.6kJ/g`

Best regards.