Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Gen Chem (6)
| Question | Answer |
|---|---|
| What are the general properties of gases? | No definite size or shape, widely separated particles, easily compressed, constant random motion, collide with container walls and other molecules |
| What are the 7 diatomic gases and their mnemonic? | H₂, N₂, F₂, O₂, I₂, Cl₂, Br₂ — mnemonic: Have No Fear Of Ice Cold Beer |
| What happens to kinetic energy and collisions when temperature increases? | ↑ Temp = ↑ kinetic energy = ↑ collisions. |
| What happens to kinetic energy and collisions when temperature decreases? | ↓ Temp = ↓ kinetic energy = ↓ collisions |
| How do solids, liquids, and gases differ in shape and volume? | Solids: fixed shape, fixed volume. Liquids: takes container shape, fixed volume. Gases: takes container shape, takes container volume |
| What is pressure? | Force of gas particles colliding with container walls |
| What happens when a gas is compressed? | Compressed: ↓ volume ↑ collisions ↑ pressure. |
| What happens when a gas is expanded? | Expanded: ↑ volume ↓ collisions ↓ pressure |
| What is held constant in Boyle's Law? | Constant: temperature and moles |
| What is held constant in Charles's Law? | Constant: pressure and moles |
| What is held constant in Avogadro's Law? | Constant: pressure and temperature |
| What is held constant in Gay-Lussac's Law? | Constant: volume and moles |
| What units must temperature always be in for gas law calculations? | Kelvin (K). Convert using: K = 273 + °C |
| Which variables are directly vs. inversely proportional to pressure? | Directly proportional: temperature (Gay-Lussac's). Inversely proportional: volume (Boyle's) |
| Which variables are directly proportional to volume? | Temperature (Charles's) and moles (Avogadro's) are both directly proportional to volume |
| What are the 5 postulates of the Kinetic-Molecular Theory of Gases? | Particles in constant random motion Combined volume of particles is negligible Particles exert no forces on one another Collisions are completely elastic (no intermolecular forces) All gases have the same average kinetic energy at a given temperature |
| Under what conditions do gases behave most ideally? | Low pressure and high temperature — both conditions minimize intermolecular forces |
| Why do gases behave more ideally at low pressure? | Particles are more spread out, leading to fewer interactions and decreased intermolecular forces |
| Why do gases behave more ideally at high temperature? | Higher kinetic energy causes particles to bounce off each other, weakening intermolecular forces |
| What are the two ideal gas constants and when is each used? | R = 0.0821 L·atm/mol·K (used when pressure is in atm). R = 8.314 L·kPa/mol·K (used when pressure is in kPa) |
| What is STP and what volume does 1 mol of any gas occupy at STP? | STP = standard temperature (273 K) and standard pressure (1 atm). 1 mol of any gas at STP = 22.4 L regardless of molecule type |
| What is Dalton's Law of Partial Pressure? | The total pressure of a gas mixture equals the sum of partial pressures of each individual gas |
| What is partial pressure? | Pressure exerted by one gas in a mixture |
| How do you calculate mole fraction? | X₁ = moles of gas 1 / total moles. Mole fraction is always between 0 and 1 |
| Under the same conditions (same P and T), what determines the density of a gas? | Molar mass only — the gas with the highest molar mass has the highest density |
| What is the difference between diffusion and effusion? | Diffusion: molecules move from high to low concentration. Effusion: gas molecules escape through a tiny hole from one container to another |
| What is the order of effusion rates by phase of matter? | Gas > Liquid > Solid (gas effuses fastest) |
| What is Graham's Law of Effusion | Effusion rate is inversely proportional to the square root of molar mass |
| Which gas effuses faster — a heavier or lighter gas? | Lighter gas effuses faster because effusion rate is inversely proportional to the square root of molar mass |
| Under the same conditions, which gas has the highest density and which has the highest effusion rate? | Highest density: heaviest gas (highest molar mass). Highest effusion rate: lightest gas (lowest molar mass). These are always opposites. |
| What is the volume conversion for liters? | 1 L = 1,000 mL = 1,000 cm³ |
| When solving a gas law problem with multiple changing variables, which law do you use? What if only pressure and volume change? | Multiple variables changing → Combined Gas Law. Only pressure and volume changing (constant T) → Boyle's Law |
Created by:
smurtab