|AP Chemistry - Graham's Law of Effusion Worksheet|
|1.||Under conditions in which the density of carbon dioxide is 1.96
g/L and that of nitrogen is 1.25 g/L, which gas will effuse more rapidly?
What will be the ratio of the rates of effusion of nitrogen to carbon dioxide?
|2.||Uranium hexafluoride is a white solid that readily passes directly
into the vapour state. At room temperature (20oC), its vapour
pressure is 16 kPa. A trace amount (about 0.7%) of the uranium in this compound
is of the type that can be used in nuclear power plants or atomic bombs. It's
called uranium-235. Essentially all of the rest, called uranium-238, is useless
for direct applications in power plants or bombs. In fact, its presence interferes.
During World War II a massive government effort was made to separate the
two kinds of uranium. Gas effusion was used because the density of the hexachloride
made from uranium-235 is 2.2920 g/L at 16 kPa and 20oC while under
the same conditions the density of the hexafluoride made from uranium-238
is 2.3119 g/L. (In the gaseous states, these compounds behave remarkably
like ideal gases.) Calculate how much more rapidly the lower-density compound
will effuse compared to the higher-density compound. (The very small difference
that you will find was actually enough, but repeated effusions were necessary.
|3.||A store receives a shipment of defective balloons. Each has a
tiny pinhole of the same size. If one balloon is filled with helium
and another is filled with air to the same volume and pressure, which balloon
will deflate faster and how much faster? The density of helium at room
temperature is 0.00016 g/mL and that of air is 0.0012 g/mL.
|4.||Natural gas pipelines cannot be kept totally free of developing
microscope leaks. Natural gas is methane, which has a density at room
temperature and 101.3 kPa of 0.654 g/L. Under these conditions the density
of hydrogen is 0.0818 g/L. This difference in density, in the light
of Graham's law, suggests a potential problem in using natural gas pipelines
for sending hydrogen if we should ever adopt hydrogen as an alternative fuel
to methane. What is this problem? Compare the rate of effusion
of hydrogen to the rate for methane.
|5.||Under the same conditions of temperature and pressure, does hydrogen
iodide or ammonia effuse faster? Calculate the relative rates
at which they effuse.
|6.||Solar energy may some day be used to split water into hydrogen
and oxygen and the hydrogen then used as a fuel. The different rates
of effusions of hydrogen and oxygen from a mixture of the two and through
a very tiny hole might be the basis of separating them. Which gas effuses
more rapidly, and by what relative amount?
|7.||What is the formula weight of a gaseous element if at room temperature
it effuses though a pinhole 2.16 times as rapidly as xenon? Which element
|8.||Compute the relative velocities of H2 and CO2
through a fine pin-hole in a barrier.
|9.||A small bicycle pump is filled with helium (He) gas. With constant
pressure, the gas is forced out through a small aperture in two seconds.
The same pump is filled with hydrogen bromide (HBr) gas.
Using the same pressure, how long will it take to force out this gas?
|10.||Calculate the relative rates of diffusion of H2(g)
and Br2(g) at the same temperatures.
|11.||A bicycle pump is filled with helium (He) gas. With constant
pressure, the gas is forced out through a small aperture in five seconds.
How long will it take to expel sulphur dioxide, SO2, from this
same pump under the same constant pressure?
|12.||An unknown gas effuses through a capillary in 60 seconds. The
same volume of hydrogen escapes in 10 seconds. Calculate the molecular mass
of the unknown gas.
|13.||Agent 86 opens a vial of knockout gas at the end of a hallway
5 m from a guard. But Agent 99 is 4 m away and is wearing a powerful
perfume, which, if the guard notices will mean immediate capture. The
knockout gas has a molar mass of 255 g/mol and takes 1.5 seconds to work.
The perfume odour has a molecule mass of 400 g/mol and will reach the guard
in 12 seconds. Will Agents 86 and 99 be caught?
|14.||Your friend has "gambler's disease." He bets you that his
2 mL of HCl gas will diffuse through a 100 cm length of glass tubing faster
than your 2 mL of NH3 gas will pass through a 130 cm length of
identical tubing. He gives you 5:1 odds that he will win. He
will increase the odds to 10:1 if you come up with a foolproof means of judging
(i) What "foolproof means" would you use to judge this race?
(ii) Who will win? Why?
(iii) If you win, how much do you bet? You need $1000.00 for the weekend.