Determine whether the process of dry ice evaporating is endothermic or exothermic and indicate the sign of ΔH.

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.

Which of the following processes for ethanol (C2H5OH) is endothermic?

Ethyl chloride (C2H5Cl), a substance used as a topical anesthetic, is prepared by reaction of ethylene with hydrogen chloride: C2H4(g) + HCl(g) → C2H5Cl(g) ΔH° = -72.3 kJ. What is the value of ΔE (in kilojoules) for the reaction, assuming no work is done other than pressure-volume work?

Given 307.5 g of hot tea at 73.5 °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 313.5 g of hot tea at 72.5 °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.