1.Which has the higher vapor pressure at constant temperature, pure water or seawater? Explain your answer.

2.Why does the vapor pressure of a liquid increase with increasing temperature?

3. A solution contains 3.5 moles of water and 1.5 moles of nonvolatile glucose (C₆H₁₂O₆). What is the mole fraction of water in this solution? What is the vapor pressure of the solution at 25C, given that the vapor pressure of pure water at 25C is 23.8 torr?

4.A solution contains 4.5 moles of water, 0.3 moles of sucrose (C₁₂H₂₂O₁₁), and 0.2 moles of glucose. Sucrose and glucose are nonvolatile. What is the mole fraction of water in this solution? What is the vapor pressure of the solution at 35C, given that the vapor pressure of pure water at 35C is 42.2 torr?

5. Calculate the molality of each of the following solutions:

a. 0.433 mol of sucrose (C₁₂H₂₂O₁₁) in 2.1 kg of water

b. 71.5 mmol of acetic acid (CH₃COOH) in 125 g of water

c. 0.165 mol of baking soda (NaHCO₃) in 375.0 g of water

6. How many moles of solute are there in the following solutions?

a. 0.750 m glucose solution made by dissolving the glucose in 10.0 kg of water

b. 0.183 m Na₂CrO₄ solution made by dissolving the Na₂CrO₄ in 900.0 g of water

c. 1.425 m urea solution made by dissolving the urea in 750.0 g of water

7.Cinnamon The distinctive aroma of cinnamon comes from cinnamaldehyde (C₉H₈O). Determine the boiling point elevation of a solution of 100 mg of cinnamaldehyde dissolved in 1.00 g of carbon tetrachloride (K_b = 5.02C/m).

8.Saccharin Determine the melting point of an aqueous solution made by adding 186 mg of saccharin (C₇H₅O₃NS) to 1.00 mL of water (density = 1.00 g/mL, K_f = 1.86 C/m).

9.Determine the boiling point of an aqueous solution that is 2.50 m ethylene glycol (HOCH₂CH₂OH); K_b for water is 0.52C/m. Assume that the boiling point of pure water is 100.00C.