Combined Gas Law: Definition, Formula & Example

An error occurred trying to load this video.

Try refreshing the page, or contact customer support.

Coming up next: Rate of a Chemical Reaction: Modifying Factors

You're on a roll. Keep up the good work!

Take Quiz Watch Next Lesson
Your next lesson will play in 10 seconds
  • 0:01 What is the Combined Gas Law?
  • 2:03 The Formula
  • 2:47 Examples
  • 4:39 Lesson Summary
Add to Add to Add to

Want to watch this again later?

Log in or sign up to add this lesson to a Custom Course.

Login or Sign up

Create an account to start this course today
Try it free for 5 days!
Create An Account

Recommended Lessons and Courses for You

Lesson Transcript
Instructor: Nissa Garcia

Nissa has a masters degree in chemistry and has taught high school science and college level chemistry.

While studying chemistry, you may have learned about the different gas laws, including Boyle's law, Charles' law, and Gay-Lussac's law. What happens if we combine all these laws together? We come up with a whole new gas law: the combined gas law, which we'll take a look at in this lesson.

What Is the Combined Gas Law?

The combined gas law makes use of the relationships shared by pressure, volume, and temperature: the variables found in other gas laws, such as Boyle's law, Charles' law and Gay-Lussac's law. Let's review the basic principles of these three laws.

Imagine you are a diver, and you begin your dive with lungs full of air. As you go deeper under water, the pressure you experience in your lungs increases. When this happens, the air inside your lungs gets squished, so the volume decreases. This is an example of Boyle's law in action, which states that the higher the pressure (P), the lower the volume (V), as shown in this image. Here, k is any constant number.

Have you ever tried putting a balloon in the refrigerator and notice that it shrinks? As the temperature of the refrigerated balloon decreases, the volume of the gas inside the balloon also decreases. When you take the balloon out of the refrigerator, it reverts to its original size, so the opposite is also true; when the temperature increases, the volume also increases. The shrinking balloon serves as a demonstration of Charles' law, which states that the higher the temperature (T), the higher the volume (V).

Imagine yourself driving down a road, which can cause the temperature to increase within your tires. As a result, the air inside the tires expands, and the pressure increases. This is an example of Gay-Lussac's law, which shows the relationship between pressure (P) and temperature (T) when the volume remains constant; as the temperature increases, the pressure also increases.

When we put Boyle's law, Charles' law, and Gay-Lussac's law together, we come up with the combined gas law, which shows that:

  • Pressure is inversely proportional to volume, or higher volume equals lower pressure.
  • Pressure is directly proportional to temperature, or higher temperature equals higher pressure.
  • Volume is directly proportional to temperature, or higher temperature equals higher volume.

The Formula

Let's take a look at the formula for the combined gas law. Here, PV / T = k shows how pressure, volume and temperature relate to each other, where k is a constant number.

The formula for the combined gas law can be adjusted to compare two sets of conditions in one substance. In the equation, the figures for pressure (P), volume (V), and temperature (T) with subscripts of one represent the initial condition, and those with the subscripts of two represent the final condition.

P1V1 / T1 = P2V2 / T2

It is important to note that the temperature should always be in Kelvin, so if the given units are in Celsius, then those should be converted to Kelvin by adding 273. We will demonstrate how this is done in the next section.


How do we use the combined gas law? Let's go over a few sample problems.

Example One: 450 mL of a gas occupies a container that has a temperature of 28°C and a pressure of 788 mmHg. What is the temperature if the volume is reduced to 50 mL at 760 mmHg? As the unit of measurement is in Celsius, remember to convert it to Kelvin.

Here, we see that the pressure decreased by a little and the volume decreased by a lot. As temperature and pressure are directly proportional to teach other, the final temperature also decreased in comparison to the initial temperature.

To unlock this lesson you must be a Study.com Member.
Create your account

Register for a free trial

Are you a student or a teacher?
I am a teacher
What is your educational goal?

Unlock Your Education

See for yourself why 10 million people use Study.com

Become a Study.com member and start learning now.
Become a Member  Back

Earning College Credit

Did you know… We have over 95 college courses that prepare you to earn credit by exam that is accepted by over 2,000 colleges and universities. You can test out of the first two years of college and save thousands off your degree. Anyone can earn credit-by-exam regardless of age or education level.

To learn more, visit our Earning Credit Page

Transferring credit to the school of your choice

Not sure what college you want to attend yet? Study.com has thousands of articles about every imaginable degree, area of study and career path that can help you find the school that's right for you.

Create an account to start this course today
Try it free for 5 days!
Create An Account