Select all that are True. Comparing a liquid and gas at the same saturation temperature, molecular kinetic energies are the same. O Comparing a liquid and gas at the same saturation temperature, molecular kinetic energy of the liquid is smaller. Molar energy of a gas (molecular KE + intermolecular PE) can be equal to molar energy (molecular KE + intermolecular PE) of a liquid for the same substance at the same saturation temperature. When a pair of molecules is at a distance where the intermolecular potential energy is negative, the intermolecular force is always negative.

Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution 6.0 g of ethylene glycol (C₂H6O2) dissolved in 200. mL of water 6.0 g of potassium sulfate (K₂SO4) dissolved in 200. mL of water 6.0 g of sucrose (C12H22011) dissolved in 200. mL of water 200. mL of pure water freezing point ✓ (choose one) 1(lowest) 2 3 4(highest) (choose one) X boiling point (choose one) (choose one) (choose one) (choose one) Ś

Determine the chemical formulas for the two compounds. Based on their structures, which compound will have the higher boiling point?

Ethanol, with ΔHvap = 40.5 kJ mol-1, has a higher ΔHvap than methanol, which is 35.2 kJ mol-1, due to its larger size and greater intermolecular forces. Because the ΔHvap for ethanol is larger, we would expect that for the two liquids to reach the same vapor pressure, the temperature for ethanol would have to be higher. If the vapor pressure is 0.0992 atm at 27.3 °C, what would the temperature be when the vapor pressure is 4.52 atm?

Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution freezing point boiling point 7.3 g of glycerin (C3H8O3) dissolved in 100. mL of water (choose one) (choose one) 7.3 g of glucose (C6H1206) dissolved in 100. mL of water (choose one) (choose one) 7.3 g of potassium iodide (KI) dissolved in 100. mL of water (choose one) (choose one) 100. mL of pure water (choose one) (choose one)

Pentane C5H12 boils at 360C at 1 atmosphere pressure. What is the molar heat of vaporization in kJ/mol if the vapor pressure of pentane at 250C is 505 torr?

Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution 7.6 g of ethylene glycol (C₂H60₂) dissolved in 500. mL of water 7.6 g of propylene glycol (C3H8O₂) dissolved in 500. mL of water 7.6 g of potassium acetate (KCH3CO₂) dissolved in 500. mL of water 500. mL of pure water freezing point (choose one) O (choose one) (choose one) (choose one) X boiling point (choose one) (choose one) (choose one) (choose one) Ś

The following compounds are liquid at -10 °C: diethyl ether, methanol, and ethylene glycol. Arrange the three compounds in order of increasing vapor pressure at -10 °C. Choose between 1 - lowest vapor pressure, 2, or 3 - highest vapor pressure. Note: Reference the Phase change properties of pure substances table for additional information. Ethylene glycol (Choose one) Methanol (Choose one) Diethyl ether (Choose one) G

Which of the following molecules has the higher AHvap (the amount of energy needed to change the substance from a liquid to a gas) and why? A They both have the same Hvap, because they have the same type of intermolecular force. AHvap is temperature dependent, so it depends on the temperature. A, because it has stronger intermolecular forces, requiring more energy to overcome the intermolecular forces. B, because it has stronger intermolecular forces, requiring more energy to overcome the intermolecular forces. Not enough information is given.

Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution freezing point boiling point 2.0 g of ethylene glycol (C2H602) dissolved in 300. mL of water (choose one) (choose one) 2.0 g of potassium acetate (KCH3CO2) dissolved in 300. mL of water (choose one) (choose one) 2.0 g of glucose (C6H1206) dissolved in 300. mL of water (choose one) (choose one) 300. mL of pure water (choose one) (choose one)