Question

Item 26 Review l Constants i Periodic Table Learning Goal: To use partial pressure in gas law calculations In a mixture of gases, the total pressure of the gas mixture is equal to the sum of the partial pressures of the individual gases. For example, if you have a mixture of helium at 2 atm and argon at 4 atm, then the total pressure of the gas inside the cylinder is 6 atm . (Figure 1) Similarly, if you know the total pressure of a gas mixture, you can use the number of moles to find the partial pressures, or the partial pressures to find the number of moles Example Problem: A mixture of N2, 02, and He gases has a total pressure of 1 atm. The partial pressures of N2 and 02 are 0.7 atm and 0.25 atm, respectively. What is the Figure 1 of 1

Answer 1

ns X2二2.7 o 0821 X 23

Now, g03-o 0 3 03 mo d . He- Now Mass = 0.303