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