(12.8)A substance is initially at 301 K and 1.01 bar (pressure unit). What phase transition occurs when the temperature changes to 201 K at constant pressure? 49.0 Liquid 167 Solid 1.01 0.05 Vapor Pressure (bar) (not to scale) O freezing O sublimation O condensation O vaporization 279 353 Temperature (K) 562

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 2.2 g of ethylene glycol (C₂H602) dissolved in 200. mL of water 2.2 g of sucrose (C12H22011) dissolved in 200. mL of water 2.2 g of potassium nitrate (KNO3) dissolved in 200. mL of water 200. mL of pure water freezing point (choose one) (choose one) (choose one) (choose one) X boiling point (choose one) (choose one) O (choose one) (choose one)

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

3. It is a quantity of heat need to convert  a mole of liquid into gas phase at a specified temperature? a. molar enthalpy  of vaporization b. molar enthalpy of boiling c. molar enthalpy of freezing d. molar enthalpy of evaporation

The following information is given for benzene, C6H6, at 1atm: AHvap(80.1 °C) = 30.7 kJ/mol boiling point = 80.1 °C specific heat liquid = 1.74 J/g°C At a pressure of 1 atm, boiling point of 80.1 °C. kJ of heat are needed to vaporize a 40.2 g sample of liquid benzene at its normal

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?

- Suppose a small sample of pure X is held at -182. °C and 0.8 atm. What will be the state of the sample (solid, liquid, or gas)?  - Suppose the temperature is held constant at -182. °C but the pressure is increased by 0.3 atm. What will happen to the sample (nothing, it will melt, it will freeze, it will boil, it will condense, it will sublime, or it will deposit)?  - Suppose, on the other hand, the pressure is held constant at 0.8 atm but the temperature is increased by 178.°C. What will happen to the sample (nothing, it will melt, it will freeze, it will boil, it will condense, it will sublime, or it will deposit)?  This all part of one question

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 6.4 g of glucose (C6H1206) dissolved in 300. mL of water (choose one) O (choose one) 6.4 g of potassium sulfate (K2SO4) dissolved in 300. mL of water (choose one) (choose one) O 6.4 g of sodium bromide (NaBr) dissolved in 300. mL of water (choose one) (choose one) O 300. mL of pure water (choose one) E (choose one) E