# carter tomlenovich

String nick = new String("hyperlisk");

System.out.println(https://hyperlisk.dev);

### Ideal Gas Mixtures

• Ideal mixtures of gases are comprised of molecules that do not interact.

• Their contrubutions simply add together.

• Consider a mixture of ideal gases in a volume V aty temperature T. For any ideal gas “X” in the mixture, we have:

• $PV = nRT -> P_x = \frac{n_xRT}{V}$

### Partial Pressure

• The total pressure of an ideal gas mixture is related to the total number of gas molecules:
• $P_{total} = \frac{n_{total}RT}{V}$
• The total number of moles is the sum of the moles for each componenet gas:
• $n_{total} = n_a + n_b …$
• Therefore the total pressure is:
• $P_{total} = \frac{n_aRT}{V} + \frac{n_bRT}{V} + \frac{n_cRT}{V} …$
• Each of these statements of the total pressure due to one gas mixture componenet as if it were alone in the vessel.
• These are called the “partial pressure” pf the component gas, $P_x$

### Dalton’s Law of Partial Pressures

• ” The total Pressure of a gas mixture is the sum of the partial pressures of the componenets of the mixture.
• $P_{total} = P_a + P_b + P_c + …$

### Mole Fractions

• The “Mole fraction” of gas A is the fraction of moles in a mixture that are of type A:
• $x_a = \frac{moles of a_a}{total moles in a mixture} = \frac{n_a}{n_{total}}$
• As a result we can easily determine partial pressure from mole fractions:
• $P_A = x_aP_{total}$