Final answer:
After burning a 0.450 g hydrocarbon sample, 24.080 kJ of energy was released. For a 5.00 g sample, 267.562 kJ of energy would be released. This calculation assumes that the energy released scales linearly with the mass of the sample.
Step-by-step explanation:
To calculate the change in energy when the hydrocarbon mixture is burned, we use the calorie meter's heat capacity and the temperature change. For the first sample of 0.450 g:
- Calorimeter heat capacity = 3440 J/°C
- Temperature rise = 7.00 °C
The energy change (q) is calculated by multiplying the heat capacity by the temperature change:
q = heat capacity × temperature change
q = 3440 J/°C × 7.00 °C = 24080 J
Convert to kilojoules by dividing by 1000:
q = 24.080 kJ
For the 5.00 g sample:
The ratio of the mass of the second sample to the first sample is:
Mass ratio = 5.00 g / 0.450 g
Mass ratio = 11.111 (rounded to three decimal places)
Since the amount of heat released is directly proportional to the mass of the sample burned, we can multiply the energy change by the mass ratio:
Energy change for 5.00 g = 24.080 kJ × 11.111
Energy change for 5.00 g = 267.562 kJ (rounded to three decimal places)