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## AP®︎/College Chemistry

### Unit 3: Lesson 4

Ideal gas law- The ideal gas law (PV = nRT)
- Worked example: Using the ideal gas law to calculate number of moles
- Worked example: Using the ideal gas law to calculate a change in volume
- Gas mixtures and partial pressures
- Worked example: Calculating partial pressures
- Ideal gas law

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# Worked example: Using the ideal gas law to calculate number of moles

AP.Chem:

SAP‑7 (EU)

, SAP‑7.A (LO)

, SAP‑7.A.1 (EK)

The ideal gas law relates four macroscopic properties of ideal gases (pressure, volume, number of moles, and temperature). If we know the values of three of these properties, we can use the ideal gas law to solve for the fourth. In this video, we'll use the ideal gas law to solve for the number of moles (and ultimately molecules) in a sample of gas. Created by Sal Khan.

## Want to join the conversation?

- At2:30, how come the unit millimeters can be used to measure pressure?(4 votes)
- If you are meaning mmHg that is measuring how much the column of mercury changed in mm due to changes in pressure.(10 votes)

- Where on KA can I learn about Torr and mmHg and pressure and other units?(3 votes)
- At5:08Sal divided by the temperature when the formula says it should be multiplied. Was there a reason for this in the video I missed?(3 votes)
- The ideal gas law says that PV = nRT. We would multiply by T if we wanted to find something like pressure of volume. However, this problem asks us to solve for the number of moles of gas, or n. To do this, you can solve for n in the equation as Sal did, and get n = PV / RT. Here, you can see that to get n, we multiply pressure and volume, and then
*divide*by temperature and R.(2 votes)

- How do we calculate the volume of a gas produced from a reaction?(1 vote)
- In this video, Sal found the number of moles of air there were. However, air is made up of many different kinds of molecules, with different numbers and types of atoms and different masses. How does this work out?(1 vote)
- Sal is using the ideal gas law which assumes the gases to be ideal. An ideal gas is composed of spherical particles which have no mass or forces of attraction to each other or the walls of the container. It's not really what the real gases are since we have a mixture of molecules in air, but using an ideal gas approximation simplifies the math and produces answers with acceptable accuracy. So here we view all moles of gas, regardless of what compound they actually are, as the same.

Hope that helps.(2 votes)

- but what is the relation between
**P1V1/T1 = P2V2/T2**&

**PV=nRT**?(1 vote)- If the number of moles of the gas stays constant then that relation holds. If PV/T = nR, where n and R are constants then, P1V1/T1 = nR and P2V2/T2 = nR. Then through the transitive property P1V1/T1 = P2V2/T2.

Hope that helps.(2 votes)

- I was wondering how to tell the number of significant figures. Isn't the original temperature given in 2 significant figures? Do we change it to three because of the conversion?(1 vote)
- In general with sig figs your answer should have no more digits than the number with the smallest number of sig figs. But the particulars depend on which mathematical operation you're performing.

If we're multiplying/dividing then we consider the digits of the entire number for sig fig purposes. If we're adding/subtracting then we only consider the digits to the right of the decimal point for sig fig purposes.**Side note**There's also rules for using exponents/logarithms but I won't cover them here because they're not relevant for the video's problem.

So before Sal performed the final calculation, he converted the temperature from °C to K. This involves adding 273.15 to the temperature in °C to do so. So mathematically this would look like: 273.15 + 21 = 294.15, but for sig fig purposes we need to look at the decimal digits. The 273.15 has two decimal digits, but the 21 has zero decimal digits so the answer should have as many decimal digits as the number with the fewest decimal digits; or zero. So the answer accounting for sig figs should be just 294 K, which is now three sig figs. Now this is only an intermediate calculation so technically we shouldn't round off before the last calculation.

When Sal performed the final calculation it was all multiplication/division. For that calculation we need to identify how many sig figs there are for all the numbers and remember that are answer should have as many as the number with the fewest sig figs. So between the numbers: 754 Torr (3 sig figs), 1.85 L (3 sig figs), 62.36 L Torr mol^-1 K^-1 (4 sig figs), and 294 K (3 sig figs); three sig figs is the smallest number of sig figs so the final answer should only have three sigs.

Hope that helps.(2 votes)

- how did he get the number 6.022x10^23?(1 vote)
- That's Avogadro's number, which is a constant and is expected to be known prior to attempting this problem.(1 vote)

- at4:00, why is he using 62.36 instead of 760? I thought you use the same units as the given pressure (in this case mm Hg)(1 vote)
- So what if you have an equation of P=nRT/V does the K-1 and mol-1 mean that there's a fraction inside of a fraction?(1 vote)
- This confused me too at first but the units on R are (atm * L)/(mol * K), with some difference depending on whether mmHG, Torr, etc are being used.(1 vote)

## Video transcript

- [Instructor] We're told an
athlete takes a deep breath, inhaling 1.85 liters of air at 21 degrees Celsius and 754 millimeters of mercury. How many moles of air are in the breath? How many molecules? So pause this video, and see if you can figure
this out on your own. All right, now let's work
through this together. So let's think about
what they are giving us and what we need to figure out. So, they are giving us a
volume, right over here. They are also giving us a
temperature, right over here. They're also giving us, I'm trying to use all of my colors here, they're giving us a pressure. And they want us to figure
out the number of moles. I'm gonna use a green color here. So they want to know, so we often use the lowercase letter, n, to represent the number of moles. And so, do we know something
that connects pressure, temperature, volume,
and the number of moles? Well, you might be thinking
of the Ideal Gas Law, which tells us that pressure times volume is equal to the number of moles, n, times the ideal gas constant, R, times temperature, T. And so we know everything
here except for n, so we can solve for n. I know what some of you are saying, "Wait, do we know R?" Well, R is a constant. And it's going to be dependent
on which units we use, and we'll figure out
which version of R we use. But that's why I gave you
this little table here, that you might see on a formula sheet, if you were taking
something like an AP exam. So we actually do know what R is. So, we just need to solve for n. So, to solve for n, you just
divide both sides by RT, and so you are going to get that n is equal to pressure times the volume over R times T, R times T. And so this is going to be equal to what? Well, our pressure is 754
millimeters of mercury. Now, over here, where
they give us the ideal gas or the different versions
of the ideal gas constants, you don't see any of them that deal with millimeters of mercury. But they do tell us that each millimeter of mercury is equal to a Torr. If you get very, very, very precise, they are slightly different. But for the purposes of a
first-year chemistry class, you can view a millimeter
of mercury as being a Torr. So, you can view the
pressure here as 754 Torr. So, let me write that down. So, this is 754 Torr. And then we're going to
multiply that times the volume. And here, they give the volume in liters in several of these, and we're probably going
to be using this one, this version of the ideal gas constant, that has liters, Torr, moles, and Kelvin. And so let's multiply times the volume, so times 1.85 liters. And then that is going to be divided by the ideal gas constant. I'll use this version
because it's using all of the units that I already have. I know what you're thinking, "Wait, the temperature's
given in degrees Celsius." But it's easy to convert from
degrees Celsius to Kelvin. You just have to add 273 to whatever you have in degrees
Celsius to get to Kelvin, because none of these are
given in degrees Celsius. And so, I will use this
ideal gas constant. So this is going to be 62.36 liter Torr liter Torr, per mole Kelvin. Mole to the negative one
is just one over mole, so I could write it like this. Kelvin to the negative one
is just one over Kelvin. And then, I'm gonna multiply
that times the temperature. So times, what is 21 degrees
Celsius in terms of Kelvin? Well, I add 273 to that, so
that's going to be 294 Kelvin. And we can validate that
the units all work out. This liter cancels out with this liter. This Torr cancels out with that Torr. This Kelvin cancels out with this Kelvin. And so, we're going to be
left with some calculation. And, it's going to be
one over one over moles, or it's essentially going to simplify to just being a certain number of moles. And so, let's get our calculator out to figure out the number
of moles in that breath. So n, I keep using
slightly different colors, so n is going to be equal to 754 times 1.85 divided by 62.36 and then, also divided by, divided by 294, is equal to this thing. And let's see how many
significant digits we have. We have three here, three
here, three here, four here. So, when we're multiplying and dividing, we just want to use the fewest
amount that I'm dealing with. So I wanna go to three
significant figures. So 0.0, one, two, three
significant figures, so 0.0761. This is going to be 0.0761. And I could say approximately
'cause I am rounding. But that's three
significant figures there. So, that's the number of
moles of air in the breath. Now, the next question is
how many molecules is that? Well, we know that each
mole has roughly 6.022 times 10 to the 23rd molecules in it, so we just have to
multiply this times 6.022 times 10 to the 23rd. So, we could write it this way. We could write 0.0761 moles, I'll write mole, times 6.022 times 10 to the 23rd molecules, molecules per mole. Now these are going to cancel out, and I'm just going to
be left with molecules. And I can just take the
number that I had before 'cause it's nice to be
able to retain precision until you have to think about
your significant figures. And so, but once again, because we did this whole calculation, we're going to wanna round everything to three significant figures. So, let's just multiply this times 6.022. EE means times 10 to the, times 10 to the 23rd, is equal to that. And, if I round to three
significant figures, because my whole calculation, that was my limiting significant figures, I have 4.58 times 10 to the 22nd. So, this is 4.58 times 10 to the 22nd molecules. Squeeze that in there, and we're done.