Barium dioxide decomposes into barium oxide and oxygen gas according to the following reaction: 2 BaO2 → 2 BaO + O2. If 37.6 grams of BaO2 decompose and 182 kJ of heat is absorbed in this process, what is the enthalpy change (ΔH) of this reaction in kJ/mol of BaO2?

When 100.0 mL of 0.200 M NaOH is mixed with 50.0 mL of 0.400 M HCl in a calorimeter, the temperature increases from 22.50 °C to 24.31 °C. Based on this temperature change, what type of reaction is occurring?

When 100.0 mL of 0.200 M NaOH is mixed with 50.0 mL of 0.400 M HF in a calorimeter, the temperature increases from 22.50 °C to 24.68 °C. Based on this temperature change, what type of reaction is occurring?

At 25°C, the heat of fusion of aluminum is 10.6 kJ/mol and the heat of sublimation is 326.4 kJ/mol. What is the heat of vaporization of aluminum at 25°C?

Barium dioxide decomposes into barium oxide and oxygen gas according to the following reaction: 2 BaO2 → 2 BaO + O2. If 27.3 grams of BaO2 decompose and 168 kJ of heat is absorbed in this process, what is the enthalpy change (ΔH) of this reaction in kJ/mol rxn?

C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l), ΔH = -1,370 kJ. For the combustion of ethanol as described above, which of the following statements is true?

Calculate the amount of heat (in kilojoules) required to vaporize 2.58 kg of water at its boiling point, given that the enthalpy of vaporization for water is 40.7 kJ/mol.

Calculate the total amount of heat needed, in joules, to convert 75.0 grams of ice at -20°C to steam at 100°C. Given: the heat of fusion of water is 6.01 kJ/mol, the heat of vaporization is 40.7 kJ/mol, and the specific heats are: ice = 2.09 J/g°C, water = 4.18 J/g°C, steam = 2.00 J/g°C.

Determine the amount of heat (in kJ) required to vaporize 25 mL of mercury at its boiling point. For mercury, ΔHvap = 56.9 kJ/mol (at 357 °C). The density of mercury is 13.6 g/mL.