Final answer:
To find the temperature change in a calorimeter during the combustion of 0.98 grams of butane, calculate the moles of butane combusted, determine the change in internal energy, then divide this energy change by the heat capacity of the calorimeter, and convert the result to Kelvin.
Step-by-step explanation:
The student is seeking to calculate the temperature change in Kelvin (K) of a calorimeter during the combustion of 0.98 grams of butane when the internal energy change for the combustion of 1 mol of butane (C4H10) is -2883 kJ. The calorimeter has a specified heat capacity of 9.75 kJ/°C.
First, we must determine the amount of butane burned in moles. The molar mass of butane (C4H10) is roughly 58.12 g/mol. Thus, to find the moles of butane combusted, we use the formula:
moles of butane = mass (g) / molar mass (g/mol) = 0.98 g / 58.12 g/mol
To calculate the change in internal energy for 0.98 grams of butane, we take the ratio of the moles of butane combusted to a mole as follows:
change in internal energy = (0.98 g / 58.12 g/mol) * (-2883 kJ/mol)
Finally, to calculate the temperature change in degrees Celsius (°C), we divide the internal energy change by the calorimeter's heat capacity and convert it into Kelvin by adding 273.15.
temperature change (°C) = change in internal energy (kJ) / Ccal (kJ/°C)
temperature change (K) = temperature change (°C) + 273.15
As for the part that mentions other combustions and the relative energy releases, these are examples given for context within chemistry coursework regarding stoichiometry and thermochemistry, which involve similar calculations to those applied to the butane combustion scenario.