A 0.589 g sample of steam at 105.1 °C is condensed into a container with 5.61 g of water at 14.8 °C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18, the specific heat of steam is 2.01, and AH vap = 40.7 kJ/mol.

Which would you expect to have the higher fusion enthalpy, N2 or I2? Explain your choice.

5-86 Using the phase diagram of water (Figure 5-20), describe the process by which you can sublime 1 g of ice at-10°C and at 1 atm pressure to water vapor at the same temperature.

How many grams of water at 0C will be melted by the condensation of 1 g of steam at 100C?

Carbon tetrachloride, CCl4, has a vapor pressure of 213 torr at 40.C and 836 torr at 80.C. What is the normal boiling point of CCl4?

Liquid butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 35.5 g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.

5-81 Compare the number of calories absorbed when 100. g of ice at 0°C is changed to liquid water at 37°C with the number of calories absorbed when 100. g of liquid water is warmed from 0°C to 37°C.

Why does sweating cool the human body?

In each of the following groups of substances, pick the one that has the given property. Justify your answer. a. highest boiling point: HBr, Kr, or Cl2 b. highest freezing point: H2O, NaCl, or HF c. lowest vapor pressure at 25C: Cl2, Br2, or I2 d. lowest freezing point: N2, CO, or CO2 e. lowest boiling point: CH4, CH3CH3, or CH3CH2CH3 f. highest boiling point: HF, HCl, or HBr g.

A quantity of ice at 0C is added to 64.3 g of water in a glass at 55C. After the ice melted, the temperature of the water in the glass was 15C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C).