How much heat (in kJ) is required to warm 11.0 g of ice, initially at -13.0 °C, to steam at 108.0 °C? The heat capacities of ice, water, and steam are 2.09, 4.18, and 2.01 J·g⁻¹·°C⁻¹, respectively. The enthalpy of fusion of ice is 334 J/g.

How much energy (in kilojoules) is released when 21.5 g of ethanol vapor at 97.0 °C is cooled to -15.0 °C? Ethanol has a melting point of -114.5 °C, boiling point of 78.4 °C, ∆Hvap = 38.56 kJ/mol, and ∆Hfusion = 4.60 kJ/mol. The molar heat capacity of ethanol is 112 J/mol·K.

How much energy (in kilojoules) is released when 32.5 g of ethanol vapor at 99.0 °C is cooled to -10.0 °C? Ethanol has a melting point of -114.5 °C, boiling point of 78.4 °C, ΔHvap = 38.56 kJ/mol, and ΔHfusion = 4.60 kJ/mol. The molar heat capacity is 113 J/(K·mol).

How much energy is released when 42.5 g of water freezes, given that the enthalpy change for freezing water is -6.01 kJ/mol?

How much energy is released when 65.8 g of water freezes, given that the enthalpy of fusion for water is 6.01 kJ/mol?

How much heat is released when one mole of steam (18.0 g) at 100.0 °C is converted to water at 25.0 °C?

If the aluminum block is initially at 25 °C, what is the final temperature of the block after the evaporation of the alcohol, assuming the heat required for the vaporization of the alcohol comes only from the aluminum block?

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) with ΔH = -890.0 kJ. Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of CH4 is burned.

Which of the following is an endothermic process?