The temperature rises from 25.00°C to 29.00°C when 3.50 g of sucrose (C12H22O11, molar mass 342.3 g/mol) undergoes combustion in a bomb calorimeter. Calculate ΔE for the combustion of sucrose in kJ/mol sucrose, given that the heat capacity of the calorimeter is 4.50 kJ/°C.

The heat of vaporization of liquid isopropyl alcohol is 159 cal/g. Calculate the energy required to vaporize 39.5 g of this compound.

The heat of vaporization of water at 100°C is 40.66 kJ/mol. Calculate the quantity of heat that is absorbed or released when 20.00 g of steam condenses to liquid water at 100°C.

When 0.418 g of pentene, C5H12, is burned in a bomb calorimeter, the temperature rises by 4.21 °C. The heat capacity of the calorimeter is 2.46 kJ/°C. Calculate the combustion energy (ΔE) for pentene, C5H12, in kJ/g.

When 1.045 g of Na2O is added to 50.0 mL of water at 25.0 °C in a calorimeter, the temperature of the water increases to 54.4 °C. Assuming that the specific heat of the solution is 4.18 J/(g·°C) and that the calorimeter itself absorbs a negligible amount of heat, calculate the heat absorbed by the solution.