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At 760. Torr, an unknown liquid boils at 239.8 K. At 205.0 K the equilibrium vapor pressure of the unknown liquid is 103.5 Torr. What is the molar enthalpy of vaporization for this liquid?

1. On a relative basis, which of these statements is/are false: 1. The stronger the intermolecular forces in a substance are, the larger is its molar heat capacity as a liquid. 2. The weaker the intermolecular forces in a substance are, the lower is its boiling point. 3. The stronger the Antermolecular forces in a substance are, the greater is its vapor pressure at a particular temperature. A. 1, 2, and 3 B. 1 only or 2 only or 3 only C. 1 and 3 D. 2 and 3 E. 1 and 2 A

A certain liquid has a vapor pressure of 92.0 Torr at 23.0 °C and 400.0 Torr at 45.0 °C. Calculate the value of AHvap for this liquid. AHvap = 52.3 Calculate the normal boiling point of this liquid. boiling point: 52 kJ/mol °C

Dry ice sublimes into carbon dioxide at -78.5 °C. What is true about the heat of the system (qsys) associated with this process?     qsys > 0     qsys < 0     qsys = 0     0< qsys < 1

Q6) A liquid is placed into a sealed vial and set on the benchtop to equilibrate at room temperature (25.0° C), and the vapor pressure is measured to be 400. torr. The flask is then heated to 42.0° C, with a new vapor pressure being measured to be 760. torr. What is the enthalpy of vaporization (in kJ/mol) for the liquid? a) 26.3 kJ/mol b) 29.5 kJ/mol c) 330 kJ/mol d) 0.98 kJ/mol

The figure below is the phase diagram of a purse substance. (I), (II) and (III) are the 3 phases of the substance, and there are 3 phase boundaries. Based on this phase diagram, which of the following statement is (are) true about this substance? a) Below 0.7 atm, the liquid phase of this substance can be formed by carefully adjusting temperature. b) The substance can be transformed from liquid to solid by applying pressure. c) The normal boiling point is between 190 K and 210 K. Pressure (in atm) 1.4 1.3 1.2 1.1 1.0 0.9 0.8 (III) 0.7 0.6- 0.5- 120 140 160 180 200 220 T (in Kelvin) O a) only O b) only O c) only O a) and b) O b) and c) O c) and a) O a), b) , and c) O None of the 3 statements is true.

Determine the normal boiling point of a liquid with vapor pressure 63.8 mmHg at 56.50°C, given that its molar heat of vaporization is 43.5 kJ/mol.

A liquid at 20.0 °C exhibits a vapor pressure of 0.555 atm. The liquid is heated to 60.0 °C. What is the new vapor pressure (in atm to three decimal places) if ΔHvap = 25.595 kJ mol–1?

Isopropyl alcohol, C3H8O, is marketed as “rubbing alcohol.” Its vapor pressure is 100 torr at 39.5°C and 400 torr at 67.8°C. Estimate the molar heat of vaporization of isopropyl alcohol

Determine the ∆Hvap for a compound that has a measured vapor pressure of 24.3 torr at 273K and 135 torr at 325K.

I am a bit unsure and confused from the particle drawings to differ on what's what

A cup of ice water is placed on the counter. The temperature of the mixture is 0 C. After 15 minutes there is still ice remaining. What is the temperature of the mixture?

4. Carbon tetrachloride, CCl4, was once used as a dry cleaning solvent, but is no longer used because it is carcinogenic. At 59.2°C, the vapor pressure of CCl4 is 58.9 kPa, and its enthalpy of vaporization is 29.82 kJ/mol. Use this information to estimate the normal boiling point (in °C) for CCl4.   °C 5. How much heat (in kJ) is required to convert 423 g of liquid H2O at 24.8°C into steam at 147°C? (Assume that the specific heat of liquid water is 4.184 J/g·°C, the specific heat of steam is 2.078 J/g·°C, and that both values are constant over the given temperature ranges. The normal boiling point of H2O is 100.0°C.)   kJ 6. From the phase diagram for water (figure below), determine the state of water at the following. (a) 34°C and 83 kPa solidliquid    gas (b) 0.01°C and 0.2 kPa solidliquid    gas (c) −10°C and 24 kPa solidliquid    gas (d) 195°C and 96 kPa solidliquid    gas (e) 42°C and 117 kPa solidliquid    gas (f) 85°C and 10 kPa solidliquid…

Two students measure the vapor pressure of the same unknown organic liquid and compare results. The first student measured a vapor pressure of 630.4 torr at 191 °C, while the second student measured a vapor pressure of 0.5570 atm at 160 °C. What is the ΔH°vap, in kilojoules per mole, for this substance?

General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning A certain liquid has a vapor pressure of 92.0 Torr at 23.0 °C and 279.0 Torr at 45.0 °C. Calculate the value of AHvap for this liquid. AHvap kJ/mol Calculate the normal boiling point of this liquid. boiling point: °C

Given the phase diagram for iodine (I2) below, predict what happens when an iodine sample is heated from 50°C to 250°C at a constant pressure of 1 atm. Note that the pressure and temperature values are just estimates.

Can you explain this problem? Where did the P1 came from? And can you redo the calculation?

At 307 K, the vapor pressure of a liquid is 15 kPa, and at 389 K, it’s vapor pressure is 121 kPa. Use this information to estimate the enthalpy of vaporization in kJ.   R= 8.314 J/(mol*K) (Please type answer)

The normal boiling point of ethyl acetate is 77.1 °C. Calculate the vapor pressure at 22.2 °C. Given: Heat of vaporization of ethyl acetate = 35.2 kJ/mol. 9.48 atm 0.106 atm 0.998 atm 0.557 atm