Ch14
For a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure
Boyle's law
The volume of a fixed mass of gas is directly proportional to its Kelvin temperature, if the pressure is kept constant
Charles's law
At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases
Dalton's law
The pressure of a gas is directly proportional to its Kelvin temperature if the volume is kept constant
Gay-Lussac's law
The rate at which a gas will effuse is inversely proportional to the square root of the gas's molar mass
Graham's law
An ideal gas CANNOT be ______. a. condensed b. heated c. compressed d. cooled
a
At high pressures, how does the volume of a real gas compare with the volume of an ideal gas under the same conditions? a. It is much greater b. It is much less c. There is no difference d. It depends on the type of gas
a
How does the gas propellant move when an aerosol can is used? a. from a region of high pressure to a region of lower pressure b. from a region of low pressure to a region of equally low pressure c. from a region of high pressure to a region of equally high pressure d. from a region of low pressure to a region of higher pressure
a
If a balloon is heated, what happens to the pressure of the air inside the balloon if the volume remains constant? a. It increases b. The change cannot be predicted c. It stays the same d. It decreases
a
If a balloon is heated, what happens to the volume of the air in the balloon if the pressure is constant? a. It increases b. The change cannot be predicted c. It stays the same d. It decreases
a
If a balloon is squeezed, what happens to the pressure of the gas inside the balloon? a. It increases b. It decreases c. It stays the same d. The pressure depends on the type of gas in the balloon
a
What happens to the pressure of a gas inside a container if the temperature of the gas decreases? a. The pressure decreases b. The pressure does not change c. The pressure increases d. The pressure cannot be predicted
a
What happens when a piston is used to decrease the volume of a contained gas? a. Gas particles become compressed b. The piston's pressure on the gas becomes greater than the pressure exerted by the gas on the piston. c. Gas particles leak out of the container d. Fewer gas particles exert a force on the piston
a
When the pressure and number of particles of a gas are constant, which of the following is also constant? a. the ratio of the volume and temperature in kelvins b. the product of the volume and temperature in kelvins c. the sum of the volume and temperature in kelvins d. the difference of the volume and temperature in kelvins
a
Which law can be used to calculate the number of moles of a contained gas? a. ideal gas law b. combined gas law c. Charles's law d. Boyle's law
a
Which of the following atoms would have the greatest velocity if each atom had the same kinetic energy? a. hydrogen b. ammonia c. chlorine d. bromine
a
Why does air escape from a tire when the tire valve is opened? a. The pressure outside the tire is lower than the pressure inside the tire b. The temperature is higher outside the tire than inside the tire c. There are more particles of air outside the tire than inside the tire d. The pressure outside the tire is greater than the pressure inside the tire
a
A box with a volume of 22.4 L contains 1.0 mol of nitrogen and 2.0 mol of hydrogen at 0°C. Which of the following statements is true? a. The partial pressure of N₂ and H₂ are equal. b. The partial pressure of N₂ is 101 kPa. c. The total pressure in the box is 101 kPa. d. The total pressure is 202 kPa.
b
As the temperature of the gas in a balloon decreases, which of the following occurs? a. The gas pressure inside the balloon increases b. The average kinetic energy of the gas decreases c. The volume of the balloon increases d. all of the above
b
At a certain temperature and pressure, 0.20 mole of carbon dioxide has a volume of 3.1 L. A 3.1 L sample of hydrogen at the same temperature and pressure ______. a. has the same mass b. contains the same number of molecules c. has a higher density d. contains the same number of atoms
b
If 4 moles of gas are added to a container that already holds 1 mole of gas, how will the pressure change inside the container? a. The pressure will not change b. The pressure will be five times higher c. The pressure will double d. The pressure will be four times higher
b
If a sealed syringe is heated, in which direction will the syringe plunger move? a. The direction cannot be predicted b. out c. in d. The plunger will not move
b
If the volume of a container of air is reduced by one-half, what happens to the partial pressure of oxygen within the container? a. It is reduced by one-fourth b. It is doubled c. It does not change d. It is reduced by one-half
b
The combined gas law relates which of the following? a. temperature and pressure only b. temperature, pressure, and volume c. pressure and volume only d. volume and temperature only
b
What happens to the partial pressure of oxygen in a sample of air if the temperature is increased? a. It decreases b. It increases c. The change cannot be determined d. It stays the same
b
Which of the following gases is the best choice for inflating a balloon that must remain inflated for a long period of time? a. neon b. argon c. hydrogen d. oxygen
b
Which of the following gases will effuse the most rapidly? a. ammonia b. hydrogen c. bromine d. chlorine
b
Why does the pressure inside a container of gas increase if more gas is added to the container? a. There is an increase in the temperature of the gas b. There is an increase in the number of collisions between particles and the walls of the container c. There is a decrease in the volume of the gas d. There is an increase in the force of the collisions between the particles and the walls of the container
b
At low temperatures and pressures, how does the volume of a real gas compare with the volume of an ideal gas under the same conditions? a. It depends on the type of gas. b. There is no difference. c. It is less. d. It is greater.
c
If oxygen is removed from a sample of air as iron rusts, what happens to the partial pressure of oxygen in the air? a. The change cannot be determined b. It stays the same c. It decreases d. It increases
c
If oxygen is removed from a sample of air as iron rusts, what happens to the total pressure of the air? a. The change cannot be determined b. It stays the same c. It decreases d. It increases
c
What does the ideal gas law allow a scientist to calculate that the other gas laws do not? a. volume b. pressure c. number of moles d. temperature
c
Why is a gas easier to compress than a liquid or a solid? a. Its volume increases more under pressure than an equal volume of solid does b. The space between gas particles is much less than the space between liquid or solid particles c. The volume of a gas's particles is small compared to the overall volume of liquid does d. Its volume increases more under pressure than an equal volume of liquid does
c
a measure of how much the volume of matter decreases under pressure
compressibility
How is the ideal gas law usually written? a. PV/nT=R b. P=nRT/V c. PV/T=nR d. PV=nRT
d
If the atmospheric pressure on Mt. Everest is one-third the atmospheric pressure at sea level, the partial pressure of oxygen on Everest is ______. a. one-sixth its pressure at sea level b. one-half its pressure at sea level c. equal to its pressure at sea level d. one-third its pressure at sea level
d
If the volume of a container of gas is reduced, what will happen to the pressure inside the container? a. The pressure will decrease b. The pressure depends on the type of gas c. The pressure will not change d. The pressure will increase
d
In general, for a gas at a constant volume, ________. a. the volume of the gas is inversely proportional to its temperature in kelvins b. the volume of the gas is directly proportional to its temperature in kelvins c. the pressure of the gas is inversely proportional to its temperature in kelvins d. the pressure of the gas is directly proportional to its temperature in kelvins
d
The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change? a. It is doubled. b. It varies depending on the type of gas c. It does not change d. It is reduced by one half
d
The volume of a gas is reduced from 4 L to 0.5 L while the temperature is held constant. How does the gas pressure change? a. It decreases by a factor of eight b. It increases by a factor of two c. It decreases d. It increases
d
Under what conditions of temperature of pressure is the behavior of real gases most like that of ideal gases? a. high temperature and high pressure b. high temperature and low pressure c. low temperature and low pressure d. low temperature and high pressure
d
What happens to the temperature of a gas when it is compressed? a. The temperature decreases b. The temperature becomes unpredictable c. The temperature does not change d. The temperature increases
d
When the Kelvin temperature of an enclosed gas doubles, the particles of the gas ________. a. decrease in average kinetic energy b. decrease in volume c. strike the walls of the container with less force d. move faster
d
When the temperature and number of particles of a gas are constant, which of the following is also constant? a. the sum of the pressure and volume b. the difference of the pressure and volume c. the ratio of the pressure and volume d. the product of the pressure and volume
d
Which of the following is constant for 1 mole of any ideal gas? a. VT/P b. PVT c. PT/V d. PV/T
d
Which of these changes would NOT cause an increase in the pressure of a contained gas? a. The temperature is increased b. The average kinetic energy of the gas is increased c. More of the gas is added to the container d. The volume of the container is increased
d
tendency of molecules to move to regions of lower concentration
diffusion
the escape of gas through a small hole in a container
effusion
PV=nRT
ideal gas law
the pressure exerted by a gas in a mixture
partial pressure