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Gas
A phase of matter with fast-moving particles.
Pressure
Force exerted per unit area by gas molecules.
Gas Laws
Relationships between pressure, volume, and temperature.
Ideal Gas Law
PV=nRT; relates pressure, volume, moles, and temperature.
Dalton's Law
Total pressure equals sum of partial pressures.
Kinetic Molecular Theory
Model explaining gas behavior based on particle motion.
Elastic Collisions
No energy loss when gas particles collide.
Average Kinetic Energy
Proportional to the Kelvin temperature of gas.
Boyle's Law
Pressure inversely proportional to volume at constant temperature.
Charles's Law
Volume directly proportional to temperature at constant pressure.
Avogadro's Law
Volume directly proportional to number of moles.
Barometer
Device measuring atmospheric pressure using mercury.
Pressure Imbalance
Difference in pressure causing eardrum to pop.
Gas Particle Motion
Gas particles move randomly and collide elastically.
Volume (V)
Space occupied by gas in a container.
Temperature (T)
Measure of average kinetic energy of gas particles.
Number of Moles (n)
Quantity of gas measured in moles.
Pressure Units
Common units include atm, mmHg, and pascals.
Effusion
Gas escaping through a tiny opening.
Diffusion
Gas spreading out to fill available space.
Pressure Factors
Depends on particle number, volume, and speed.
Gas Mixtures
Homogeneous combinations of different gas types.
Boyle's Law
Volume inversely proportional to pressure at constant temperature.
Charles's Law
Volume directly proportional to temperature at constant pressure.
Kinetic Molecular Theory
Gas particles in constant motion influence pressure.
Avogadro's Law
Volume proportional to number of moles at constant temperature.
Ideal Gas Law
PV = nRT relates pressure, volume, and temperature.
Gas Constant (R)
Constant used in Ideal Gas Law equations.
Pressure (P)
Force exerted per unit area by gas collisions.
Volume (V)
Space occupied by a gas, measured in liters.
Moles (n)
Quantity of gas measured in number of particles.
Standard Conditions
Agreed conditions for reporting gas measurements.
Absolute Temperature
Temperature measured from absolute zero in Kelvin.
Gas Expansion
Increase in gas volume with temperature rise.
Pressure Drop
Decrease in pressure causes gas volume to increase.
Collision Frequency
Rate at which gas particles collide with walls.
Force per Unit Area
Definition of pressure in gas systems.
Volume Calculation
Determining gas volume using pressure and temperature.
Temperature Conversion
Change Celsius to Kelvin for gas law calculations.
Gas Behavior
Describes how gases respond to changes in conditions.
Gas Sample
Specific quantity of gas used in calculations.
Closed Vessel
Container where gas volume and pressure are measured.
Gas Measurement
Quantitative assessment of gas properties under conditions.
Standard Conditions
Conditions for gas measurements: 1 atm, 0°C, 273 K.
Molar Volume
Volume of one mole of gas at STP: 22.4 L.
Gas Density
Density calculated as grams per volume (d = g/V).
Ideal Gas Law
PV = nRT, relates pressure, volume, temperature, moles.
Partial Pressure
Pressure exerted by a single gas in a mixture.
Mole Fraction (χa)
Ratio of moles of component to total moles.
Vapor Pressure
Pressure of water vapor at a given temperature.
Collecting Gases
Gases displace water, causing vapor pressure issues.
Gas Mixture
Combination of different gases, like dry air.
Diatomic Gas
Gas composed of two atoms, e.g., O₂, N₂.
Molar Mass Calculation
Determined using ideal gas law parameters.
Gas Volume at STP
1 mole occupies 22.4 L at standard conditions.
Temperature Conversion
0°C equals 273 K for gas calculations.
Pressure Conversion
1 atm equals 760 torr for pressure measurements.
Density of Gas
Mass per unit volume, crucial for calculations.
Gas Sample Measurement
Volume, temperature, and pressure needed for analysis.
Total Pressure Calculation
Sum of individual gas pressures in a mixture.
Oxygen Collection Experiment
Pressure and volume measured to find gas mass.
Solid CO2 Vaporization
Solid CO2 turns to gas, affecting pressure.
Water Vapor in Gas
Affects total pressure when collecting gases.
Vapor Pressure
Pressure exerted by vapor in equilibrium.
Ideal Gas Law
PV=nRT; relates pressure, volume, temperature, moles.
Stoichiometry
Relationship between reactants and products in reactions.
Nitric Acid Formation
3NO2 + H2O → 2HNO3 + NO reaction.
Hydrogen Gas Collection
240.0 ml of H2 at 30.0 °C and 1.032 atm.
Vapor Pressure of Water
Pressure of water vapor at specific temperature.
Kinetic Energy
Depends on mass and velocity of gas molecules.
Root Mean Square Velocity
Average velocity of gas particles in m/s.
Molecular Speed
Speed of gas molecules related to mass.
Temperature Effect
Higher temperature increases molecular velocity distribution.
Diffusion
Molecules spreading from high to low concentration.
Effusion
Molecules escaping through a small hole.
Graham's Law of Diffusion
Rate ratio of effusion inversely proportional to molar mass.
Real Gases
Do not behave ideally at high pressure, low temperature.
Deviation Due to Pressure
Molar volume increases beyond ideal gas predictions.
Finite Volume of Gas Particles
Real gas volume larger than ideal gas volume.
Deviation Due to Temperature
Pressure lower than ideal gas at low temperatures.
Intermolecular Attractions
Forces between molecules affecting gas behavior.
Van der Waals Equation
Modified ideal gas equation for real gas behavior.
Boyle's Law
Pressure inversely proportional to volume at constant temperature.
Avogadro's Law
Volume directly proportional to moles at constant temperature and pressure.
Dalton's Law of Partial Pressures
Total pressure equals sum of individual gas pressures.
