Dry nitrogen gas is bubbled through liquid benzene (C6 H6 ) at 23.0°C. From 140.0 L of the gaseous mixture of nitrogen and benzene, 25.0 g benzene is condensed by passing the mixture through a trap at a temperature where nitrogen is gaseous and the vapor pressure of benzene is negligible. What is the vapor pressure of benzene at 23.0°C? Vapor pressure = torr Submit Answer Try Another Version 8 item attempts remaining

Define critical temperature and critical pressure. In terms of the kinetic molecular theory, why is it impossible for a substance to exist as a liquid above its critical temperature?

In the northern United States, summer cottages are usually closed up for the winter. When doing so, the owners winterize the plumbing by putting antifreeze in the toilet tanks, for example. Will adding 525 g of HOCH2CH2OH to 3.00 kg of water ensure that the water will not freeze at 25 C?

A 1.50-g sample of methanol (CH3OH) is placed in an evacuated 1.00-L container at 30 C. (a) Calculate the pressure in the container if all of the methanol is vaporized. (Assume the ideal gas law, PV = nRT.) (b) The vapor pressure of methanol at 30 C is 158 torr. What mass of methanol actually evaporates? Is liquid in equilibrium with vapor in the vessel?

Why do liquids have a vapor pressure? Do all liquids have vapor pressures? Explain. Do solids exhibit vapor pressure? Explain. How does vapor pressure change with changing temperature? Explain.

The normal boiling point of SO2 is 263.1 K and that of NH3 is 239.7 K. At −40 °C, would you predict that ammonia has a vapor pressure greater than, less than, or equal to that of sulfur dioxide? Explain.

Define the following and give an example of each: (a) dispersion force (b) dipole-dipole attraction (c) hydrogen bond

A tank of gas at 21C has a pressure of 1.0 atm. Using the data in the table, answer the following questions. Explain your answers. a If the tank contains carbon tetrafluoride, CF4, is the liquid state also present? b If the tank contains butane, C4H20, is the liquid state also present?

In an experiment, 20.00 L of dry nitrogen gas, N2, at 20.0C and 750.0 mmHg is slowly bubbled into water in a flask to determine its vapor pressure (see the figure on next page). The liquid water is weighed before and after the experiment, from which the experimenter determines that it loses 353.6 mg in mass. Answer the following questions. a How many moles of nitrogen were bubbled into the water? b The liquid water diminished by how many moles? What happened to the liquid? c How many moles of gas exit the flask during the experiment? What is the partial pressure of nitrogen gas exiting? The total gas pressure is 750.0 mmHg. d From these data, calculate the vapor pressure of water at 20C. Does this agree with what you expect?

What are intermolecular forces? How do they differ from intramolecular forces? What are dipole-dipole forces? How do typical dipole-dipole forces differ from hydrogen bonding interactions? In what ways are they similar? What are London dispersion forces? How do typical London dispersion forces differ from dipole-dipole forces? In what ways are they similar? Describe the relationship between molecular size and strength of London dispersion forces. Place the major types of intermolecular forces in order of increasing strength. Is there some overlap? That is, can the strongest London dispersion forces be greater than some dipole-dipole forces? Give an example of such an instance.