The following liquids have about the same molar mass. The vapor pressure of each was measured in the open-ended manometer shown below. JU Arrange the liquids in order of decreasing height of the mercury column, designated as h in the image. Rank from largest to smallest height of the mercury column, h. To rank items as equivalent, overlap them. ► View Available Hint(s) CH3CH₂CH₂CHCH3 I NH2 Largest height CH3CH₂CH₂CH₂CH₂-NH₂ Reset CH3CH₂CH₂CH₂ OCH3 CH3CH₂CH₂CH₂CH₂CH3 Help Smallest height

The following liquids have about the same molar mass. The vapor pressure of each was measured in the open-ended manometer shown below. JU Arrange the liquids in order of decreasing height of the mercury column, designated as h in the image. Rank from largest to smallest height of the mercury column, h. To rank items as equivalent, overlap them. ► View Available Hint(s) CH3CH₂CH₂CHCH3 I NH2 Largest height CH3CH₂CH₂CH₂CH₂-NH₂ Reset CH3CH₂CH₂CH₂ OCH3 CH3CH₂CH₂CH₂CH₂CH3 Help Smallest height

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter10: Solids, Liquids, And Phase Transitions

Section: Chapter Questions

Problem 63AP

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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?
ook at Fig. 14.2. Why doesn't temperature increase continuously ever time? That is, why does the temperature stay constanl for periods of time?
5-106 The normal boiling point of hexane, C6H14, is 69°C, and that of pentane, C5H12, is 36°C. Predict which of these compounds has a higher vapor pressure at 20°C.
he following demonstration takes place in a two-step process: rst, solid calcium carbide (CaC2j)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. Second the acetylene gas produced is then ignited with a match, causing the combustion reaction of acetylene with oxygen gas to produce gaseous carbon dioxide and gaseous water. Write the balanced equations for each reaction that is occurring, including all phases. If a 100.0gsample of calcium carbide (CaC2)is initially reacted with 50.0gof water, which reactant is limiting? Now imagine that the final gases produced are collected in a large bulkier and allowed to cool to room temperature. Using the information from part b ( l00.0gof Cec2reacting with 50.0gof H2O), how many liters of carbon dioxide gas were produced in the balloon at a pressure of 1.00atm and 25C?
Gases that cannot be liquefied at room temperature merely by compression are called permanent gases. How could you liquefy such a gas?
Helium condenses to a liquid at 4.224 K under atmospheric pressure and remains a liquid down to the absolute zero of temperature. (It is used as a coolant to reach very low temperatures.) The vapor pressure of liquid helium at 2.20 K is 0.05256 atm. Calculate the volume occupied by 1.000 mol helium vapor under these conditions and compare it with the volume of the same amount of helium at standard temperature and pressure.
On the basis of intermolecular attractions, explain the differences in the boiling points of n butane (1 C) and chloroethane (12 C), which have similar molar masses.
A syringe at a temperature of 20 C is filled with liquid ether in such a way that there is no space for any vapor. If the temperature is kept constant and the plunger is withdrawn to create a volume that can be occupied by vapor, what would be the approximate pressure of the vapor produced?
In each of the following groups of substances, pick the one that has the given property. Justify your answer. a. highest boiling point: HBr, Kr, or Cl2 b. highest freezing point: H2O, NaCl, or HF c. lowest vapor pressure at 25C: Cl2, Br2, or I2 d. lowest freezing point: N2, CO, or CO2 e. lowest boiling point: CH4, CH3CH3, or CH3CH2CH3 f. highest boiling point: HF, HCl, or HBr g.
Carbon tetrachloride, CCl4, has a vapor pressure of 213 torr at 40.C and 836 torr at 80.C. What is the normal boiling point of CCl4?
How many grams of water at 0C will be melted by the condensation of 1 g of steam at 100C?
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.

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