a. The temperature inside a pressure cooker is 124°C. Calculate the vapor pressure of water inside the pressure cooker. The enthalpy of vaporization of water is 40.7 kJ/mol. Vapor pressure = atm b. What would be the temperature inside the pressure cooker if the vapor pressure of water was 2.70 atm? The enthalpy of vaporization of water is 40.7 kJ/mol. Temperature °C

11. At the end of a cooking cycle, a pressure cooker contains a mixture of water, steam, and food at a temperature of 120°C and 1.5 atm of pressure. The pressure is valve is opened and the pressure decreases, which alters water's boiling point and causes the contents of the pressure cooker to cool rapidly. Which statement best explains why the contents cooled rapidly after the pressure was released? A. Water lost heat as it vaporized. B. Water absorbed heat as it vaporized. C. Water lost heat as it condensed. D. Water absorbed heat as it condensed.

A chemist determined vapor pressures of an unknown substance at different temperatures. The data was plotted as ln(P) vs 1/T (temperature in Kelvin). What is △H∘vap of this substance in kJ/mol?

In the Pressure vs Temperature phase diagram of a substance X, the triple point exists at p = 5 atm and T= 25 °C. Which of the following statements is true regarding substance X? A. At atmospheric pressure, an increase in temperature would cause X to undergo a phase transition from a solid state to a liquid state. B. At atmospheric pressure, an increase in temperature would cause X to undergo a phase transition from a solid state directly to a gaseous state. C. At atmospheric pressure, an increase in temperature would cause X to undergo a phase transition from a liquid state to a gaseous state. D. At atmospheric pressure, a decrease in temperature would cause X to undergo a phase transition from a liquid state to a solid state. E. At atmospheric pressure, a decrease in temperature would cause X to transition from a gaseous state to a liquid state. ndergo a phase

Use the observation in the first column to answer the question in the second column. observation At 1 atm pressure, Substance E boils at 11. °C and Substance F boils at 30. °C. At 37 °C, Substance C has a vapor pressure of 89. torr and Substance D has a vapor pressure of 79. torr. The enthalpy of vaporization of Substance A is smaller than that of Substance B. question Which has a higher vapor pressure? Substance E Substance F Neither, E and F have the same vapor pressure. It's impossible to know without more information. Which has a higher enthalpy of vaporization? Substance C Substance D Neither, C and D have the same enthalpy of vaporization. It's impossible to know without more information. At any temperature where both substances are liquid, which has the higher vapor pressure? Substance A Substance B Neither, A and B have the same vapor pressure. It's impossible to know without more information. X Ś

1. Freon-12 (CCl2F2) is banned as a refrigerant because it is harmful to the ozone. a. Sketch the phase diagram of CCl2F2 using the physical constants below Normal boiling point = -29.8 °C Normal melting point = -158 °C Critical temperature = 112 °C Critical pressure = 40.8 atm Triple point (2.42 ×10-6 atm, -157 °C) b. Calculate the heat required to bring 10.0g CCl2F2 from -29.8 °C as a liquid to the gas phase at 10.0 °C. (molar mass 120.91 g/mol) Cs (gas) = 0.074 kJ/mol·K AHvap = 20.1 kJ/mol AHfus = 4.14 kJ/mol

The atmospheric pressure in Ogden, Utah is 646 mm Hg. The boiling point of water here will be a. less than 100oC b. 100oC c. more than 100oC

The vapor pressure of Substance X is measured at several temperatures: temperature vapor pressure 4. °C 0 16. °C 28. °C 0.0584 atm 0.0961 atm 0.152 atm Use this information to calculate the enthalpy of vaporization of X. Round your answer to 2 significant digits. Be sure your answer contains a correct unit symbol. x10 ロ・ロ X I olo Ś

The vapor pressure of pure water at 35°C is 42.2 mm Hg. What is the vapor pressure of a mixture of 7.5 g sucrose (C12H22011) and 42.5 g water? a. 21.8 mm Hg O b. 41.8 mm Hg O c. 35.9 mm Hg d. 40.6 mm Hg O e. 7.45 mm Hg

B. Explain why the maximum vapor pressure and standard enthalpy of vaporization are different for the morning low temperature and the afternoon high temperature in the month of August in Philadelphia. a. Having trouble? Review questions from Chapter 10: 35, 37, and 47. Temperature Vapor Pressure Enthalpy of Vaporization Morning Low 70 °F 18.7 mmHg 44.16 kJ/mol Afternoon High 87 °F 33.7 mmHg 43.75 kJ/mol