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?

Given 393.0 g of hot tea at 81.0 °C, what mass of ice at 0 °C must be added to obtain iced tea at 12.5 °C? The specific heat of the tea is 4.18 J/(g·°C), and ΔHfusion for ice is +6.01 kJ/mol.

Given 414.5 g of hot tea at 73.0 °C, what mass of ice at 0 °C must be added to obtain iced tea at 12.0 °C? The specific heat of the tea is 4.18 J/(g°C), and ΔHfusion for ice is +6.01 kJ/mol.

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 65.8 g of water freezes, given that the enthalpy of fusion for water is 6.01 kJ/mol?

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 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?