1. The effect of adding/removing a gas
2. The effect of changing the size of a container
3. The effect of heating or cooling a gas
4. Real vs. ideal gases
5. Dalton's Law (partial pressure) [Practice ] [Reference]
6. Boyle's Law (pressure-volume relationship) [Reference]
7. Charles' Law (temperature-volume relationship) [Reference]
8. Gay Lussac's Law (temperature-pressure relationship) [Reference]
9. Combined Gas Law [Reference]
10. Ideal Gas Law [Reference]
11. Departures from the Gas Laws [Reference]
12. Diffusion and Graham's Law [Reference]

Chapter 10

10-1 The Effect of Adding or Removing Gas

- Adding gas particles to a closed container increases pressure.

10-2 The Effect of Changing the Size of the Container

- The size of the container and the pressure contained within it are inversely proportional. I.e., the larger the container, the less pressure within it, and vice versa.

10-3 The Effect of Heating or Cooling a Gas

- Temperature and pressure are directly proportional. I.e., the higher the temperature, the higher the pressure.

10-4 Real vs. Ideal Gases

- Ideal gases are only theoretical.

Note: The following Gas Laws can all be found in Chempire's Online Gas Law Guide --------LLLLLLLLLIIIIIIIINNNNNNNNNNKKKKKKK_----------------

10-5 Dalton's Law of Partial Pressure

- P(total) = P(1) + P(2) + ....

10-6 Boyle's Law for Pressure-Volume Changes

- P(initial) x V(initial) = P(final) x V(final)

- P(initial)/P(final) = V(final)/V(initial)

10-7 Charles' Law for Temperature-Volume Changes

- V(initial)/T(initial) = V(final)/T(final)

- V(initial) x T(final) = T(initial) x V(final)

10-8 Gay-Lussac's Law for Temperature-Pressure Changes

- P(initial)/T(initial) = P(final)/T(final)

- P(initial) x T(final) = T(initial) x P(final)

10-9 The Combined Gas Law

- This is the only one you really need to memorize; all the others can be derived from it by holding one of the variables (P, V, or T) constant.

- [ P(initial) x V(initial) ] / T(initial) = [ P(final) x V(final) ] / T(final)

- T(final) x P(initial) x V(initial) = T(initial) x P(final) x V(final)

10-10 The Ideal Gas Law (pivnirt)

- P x V = n x R x T

- n = moles, R = 0.0821 when using atm's with P, 62.4 when using mm Hg with P, 8310 when using Pa with P.

10-11 Departure from the Gas Laws

- Given that ideal gasses do not exist in nature (or in the laboratory for that matter), the Ideal Gas Law is not always correct. However, for stoichiometric purposes, we will assume that it is.

10-12 Diffusion and Graham's Law

- Diffusion: gas particles will move apart from each other until their concentration is the same throughout the container.

- Graham's Law of Effusion: The rate of effusion of a gas is inversely proportional to the square root of its formula mass.

- Graham's Law applies to diffusion as well.

Go to Chapter: 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20