Final answer:
To calculate the change in internal energy (∆E) in kJ/mole for the combustion of 1.00 g of butane, we find the heat released by multiplying the calorimeter's heat capacity by the temperature change, then divide by the number of moles of butane.
Step-by-step explanation:
To calculate the change in internal energy, ∆E, associated with the combustion of butane (C4H10), we use the following formula:
∆E = Ccal × ∆T
Where Ccal is the heat capacity of the calorimeter, and ∆T is the change in temperature.
Given that Ccal = 6.00 kJ/°C and ∆T = 8.3 °C, we can find the total heat released by the combustion process in the calorimeter:
∆E = 6.00 kJ/°C × 8.3 °C = 49.8 kJ
However, to express ∆E in kJ/mol, we need to find how many moles of butane correspond to 1.00 g. The molar mass of butane is approximately 58.12 g/mol (derived from the atomic masses of carbon and hydrogen). Thus, the number of moles of butane is:
moles of butane = mass (g) / molar mass (g/mol) = 1.00 g / 58.12 g/mol ≈ 0.0172 mol
Finally, to find the change in internal energy per mole, we divide the total heat released by the number of moles:
∆E per mole = 49.8 kJ / 0.0172 mol ≈ 2895.35 kJ/mol