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biochem 1100 tri-c
Chap. 7 gases
| Question | Answer |
|---|---|
| Kinetic molecular theory of gases | Gas particles are small; move randomly & rapidly; gas particles are not attracted to each other; actual volume of molecules is small; energy is propotional to the Kelvin temperature; gas particles move in straight paths |
| Gas - pressure (P) | The force exerted by gas against the walls of the container; The Atmospheric pressure is measured in units "atmosphere" (atm) millimeters of mercury (mm Hg) |
| Volume (V) | Volume of gas equals the conatiner in which it is placed; measured in units of liters (L) and milliliters (mL) |
| Temperature (T) | Temperature of a gas affects its kinetic energy - use Kelvin to measure temp. of a gas |
| Amount of Gas (n) | Usually, the amount of gas is measured by its mass (grams) |
| Pressure (equation) | Pressure (P) = Force/area |
| Atmospheric pressure | 1. Air particles have mass, they exert pressure - measured with a barometer |
| Barometer - how does it work | Pressure exerted by gases in atmospher is equal to the downward pressure of a mercury column in a closed glass tube |
| What is 1 atmosphere? | 1 atm = 760 mm Hg = 760 torr |
| What is a torr? | Name for Torricelli, the inventor of the barometer |
| Boyle's Law | P1(V1) = P2(V2) - As pressure increases, volume decreases and vice versa |
| Boyle's Law ("boy"cott law) | INVERSE relationship between Pressure and Volume |
| Charles' Law | Volume of a gas change directly with a change in Kelvin temperature |
| Charles' Law & "Kelva-milla" | The is a direct relationship between Pressure and "Kelva-milla" - degrees Kelvin - |
| Charles Law (equation) | V1 divided by T1 = V2 divided by T2 |
| Avogadro's Law (gases) | Avogardro's Law for gases - the volume of a gas is directly related to the number of moles of a gas (common sense -the more gas, the more volume) |
| STP - standard temperature and standard pressure | Standard pressure is 0 degrees Centigrade - 273 K; standard pressure is 1 atmosphere (760 mm Hg) |
| Ideal Gas Law (has four elements) | Ideal Gas Law- expresses relationship between Pressure (P), Volume (V), temperature (T) and amount of a gas (n) |
| Ideal Gas Law (equation) | P(V) divided by n(T) = R |
| Ideal gas law (units of measure) | Pressure (P) - atm or mm Hg; Volume (V) - L; Amount (n) - moles; Temperature (T) Kelvin |
| Partial Pressure (Dalton's Law) | When gases are combined, it is the number of gas molecules, not the kind of gas, which determine pressure |
| Dalton's Law - equation | P(total) = P(one) + P(two) [just keep adding moles of gas] |
| Molar volume (gas) | A volume of 22.4 L occupied by 1 mole of a gas at STP conditions of 0degres Centigrade (273 K) and 1 atm |
| What is the "standard" temperature for gas under the ideal gas law? | 0 degrees centigrade (273 Kelvin) |
Created by:
walterina4327