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Assuming the volume is held constant, what happens to the pressure of a gas when the absolute temperature doubles?
 
It is doubled.
 
It remains unchanged.
 
It is halved.
 
It is quadrupled.
Temperature is a measure of:
 
The average kinetic energy of the particles in a substance.
 
The number of particles a substance has.
 
The amount of heat a substance has.
 
The average potential energy of the particles in a substance
Which Celsius temperature is equal to 310 K?
 
37 degrees Celsius
 
583 degrees Celsius
 
285 degrees Celsius
 
310 degrees Celsius
A balloon has an initial volume of 150 mL at 25 degrees Celsius. If the temperature is increased to 75 degrees Celsius, what is the final volume?
 
175 mL
 
50 mL
 
150 mL
 
450 mL
What is the name of the sum of atomic masses (for molecular compounds) in a chemical formula?
 
molecular mass
 
formulaic mass
 
atomic mass
 
total mass
What is mass?
 
the amount of matter in an object
 
the volume of an object
 
the weight of an object
 
none of these are correct
If a 22.4 L container is holding 1.00 mole of a gas at 273 kelvins, then what is its pressure?
 
1.00 atm
 
22.2 atm
 
2.00 atm
 
22.4 atm
Assuming pressure and temperature are held constant, then what happens to the volume of a non-rigid container when the number of molecules in the container is doubled?
 
The volume doubles.
 
The volume stays the same.
 
It decreases to half its original volume.
 
There is not enough information given to determine this.
In the van der Waals equation, what does a represent?
 
The attraction between the gas molecules
 
The volume of the gas molecules
 
The number of gas particles in moles
 
The ambient temperature
Avogadro's law shows the relationship between _____.
 
volume and number of particles
 
temperature and pressure
 
pressure and number of particles
 
temperature and number of particles
A container has a volume of 53.9 L. Assuming it is at STP, how many moles of gas particles does it contain?
 
2.41 mol
 
0.416 mol
 
1,200 mol
 
76.3 mol
In the ideal gas equation, what does R represent?
 
The ideal gas constant
 
Pressure
 
Number of moles
 
Temperature
If you know the temperature, volume, and pressure of a gas, how would you rearrange the ideal gas equation to find the number of moles?
 
Divide PV by both T and R.
 
Multiply PV by both T and R.
 
Divide PV by T only.
 
Divide PV by n.
If someone is measuring pressure, they might use any of the following units EXCEPT _____.
 
Pounds
 
Atmospheres
 
Torr
 
Millimeters of mercury
What does b represent in the van der Waals equation?
 
The volume of the gas molecules
 
The volume of the container
 
The volume of the container not filled by the gas
 
The volume of the gas overall
Under non-ideal conditions, why was the pressure lower using the van der Waals equation?
 
The attraction between the molecules increases.
 
The pressure was greater.
 
The attractive forces between the molecules makes em larger
 
The attractive forces between the molecules makes em smaller
A sample of hydrogen has a volume of 25 L under a pressure of 5 atm. What will the pressure of this gas be if the volume were decreased to 5 L?
 
25 atm
 
5 atm
 
10 atm
 
15 atm
1000 mL of a gas at 15 atm is compressed to 500 mL. What is its new pressure?
 
30 atm
 
5 atm
 
3 atm
 
2 atm
Which of the following is TRUE about most gases?
 
They expand to completely fill their container.
 
Their particles are very close together.
 
They have a fixed volume.
 
All of their particles are the same size.
Why would a scientist have difficulty observing the behavior of an ideal gas?
 
Because an ideal gas is theoretical, and hence not real.
 
Because all ideal gases are invisible.
 
Because an ideal gas cannot be compressed.
 
Because an ideal gas is made of molecules that cant be seen
Why can't all of the gas particles in a container have very high or very low speeds?
 
Because as particles collide, a gain in kinetic energy other
 
Because as particles collide they both increase their energy
 
Because there is not enough pressure inside of a closed cont
 
Because there is not enough pressure inside
What does the Maxwell-Boltzmann curve tell us?
 
The probability of a particle's speed
 
he probability of massive particles
 
The probability of a particle's direction
 
The probability of a particle's curve


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