Science, Tech, Math › Science Dalton's Law Calculation Example Worked Example of Dalton's Law of Partial Pressure Problem Share Flipboard Email Print You can apply Dalton's Law to calculate pressure of a gas, such as a mixture of gases in a balloon. Lauren Hillebrandt / Getty Images Science Chemistry Basics Chemical Laws Molecules Periodic Table Projects & Experiments Scientific Method Biochemistry Physical Chemistry Medical Chemistry Chemistry In Everyday Life Famous Chemists Activities for Kids Abbreviations & Acronyms Biology Physics Geology Astronomy Weather & Climate By Anne Marie Helmenstine, Ph.D. Chemistry Expert Ph.D., Biomedical Sciences, University of Tennessee at Knoxville B.A., Physics and Mathematics, Hastings College Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. She has taught science courses at the high school, college, and graduate levels. our editorial process Facebook Facebook Twitter Twitter Anne Marie Helmenstine, Ph.D. Updated September 09, 2019 Dalton's Law of Partial Pressures, or Dalton's Law, states that the total pressure of a gas in a container is the sum of the partial pressures of the individual gases in the container. Here is a worked example problem showing how to use Dalton's Law to calculate the pressure of a gas. Review Dalton's Law Dalton's Law of Partial Pressures is a gas law that can be stated: Ptotal = P1 + P2 + P3 + ... Pn where P1, P2, P3, Pn are the partial pressures of the individual gases in the mixture. Example Dalton's Law Calculation The pressure of a mixture of nitrogen, carbon dioxide, and oxygen is 150 kPa. What is the partial pressure of oxygen if the partial pressures of the nitrogen and carbon dioxide are 100 kPA and 24 kPa, respectively? For this example, you can simply plug the numbers into the equation and solve for the unknown quantity. P = Pnitrogen + Pcarbon dioxide + Poxygen150 kPa = 100 kPa + 24 kPa + PoxygenPoxygen = 150 kPa - 100 kPa - 24 kPaPoxygen = 26 kPa Check your work. It's a good idea to add up the partial pressure to make sure the sum is the total pressure!