Gases and Gas Laws Quiz

A gas has no fixed boundaries and quickly fills its container.

Measures the hotness of an object; 0K is absolute zero.

Temperature scale with freezing point 0°C and boiling point 100°C of water.

Force exerted by a gas on a unit area.

At constant temperature, gas volume is inversely proportional to pressure.

Standard Temperature and Pressure: 273K and 100,000 Pa.

Gas volume is measured in cubic meters (m³), cubic centimeters (cm³), or liters (L).

Pressure is measured in Pascals (Pa), kilopascals (kPa) or hectopascals (hPa).

pV = k, where p is pressure, V is volume, and k is a constant related to temperature.

V/T = k, where V is volume, T is temperature (in Kelvin), and k is a constant related to pressure.

At constant pressure, the volume of a fixed mass of gas is directly proportional to its temperature measured on the Kelvin scale.

A temperature scale where 0 Kelvin represents absolute zero, the theoretical absence of thermal energy.

The theoretical temperature at which all molecular motion stops.

A relationship where if one variable increases, the other increases by the same factor.

A relationship where if one variable increases, the other decreases by the same factor.

Relates the pressure, volume, and temperature of a gas. It combines Boyle's Law and Charles' Law into one equation.

𝑝1 𝑉1 / 𝑇1 = 𝑝2 𝑉2 / 𝑇2, where p1, V1, and T1 are the initial pressure, volume, and temperature and p2, V2, and T2 are the final pressure, volume, and temperature.

States that the volumes of reacting gases and gaseous products are in the ratio of small whole numbers, as long as the temperature and pressure are kept constant.

States that equal volumes of gases contain equal numbers of molecules, as long as the temperature and pressure remain the same.

The volume occupied by one mole of a gas at a specific temperature and pressure.

The Combined Gas Law equation can be used to calculate a missing final condition (pressure, volume, or temperature) of a gas when given initial and two final conditions.

For Gay-Lussac's Law to be valid, the volumes of reacting gases and gaseous products must be measured at the same temperature and pressure.

A liquid that easily evaporates at room temperature.

The combined mass of the conical flask, cap, rubber band, and any remaining liquid inside.

The mass of the volatile liquid that has evaporated and filled the flask.

The volume of the flask, determined by filling it with water and measuring the water transferred.

The pressure exerted by the air surrounding the flask.

The pressure exerted by the vaporized volatile liquid inside the flask.

The pinhole in the flask allows vapor to escape until the pressure inside matches the pressure outside.

The mass of one molecule of a substance relative to the mass of a carbon-12 atom.

Avogadro's Law states that equal volumes of ideal gases contain the same number of molecules at constant temperature and pressure.

The kinetic theory of gases assumes that gas particles are in constant random motion and have negligible volume compared to the container they occupy.

Real gases deviate from ideal gas behavior due to intermolecular forces and finite particle volume.

To determine the number of moles of a gas from its atoms, divide the number of atoms by Avogadro's number (6.022 x 10^23) to find the number of molecules and then divide by Avogadro's number again to get the number of moles.

Mass spectrometry is a technique used to determine the relative molecular mass of substances, regardless of their volatility or state of matter.

A gas that perfectly obeys all the assumptions of the kinetic theory of gases under all conditions of temperature and pressure. It is theoretical and does not exist in reality.

The kinetic theory of gases describes ideal gas behavior based on assumptions like particles in constant random motion, negligible particle volume compared to space, and collisions being perfectly elastic.

1. There are attractive forces between gas particles, contrary to the theory's assumptions. 2) The volume of gas particles is not entirely negligible compared to the space between them.

The ideal gas law equation is pV = nRT, where p is pressure, V is volume, n is the number of moles, R is the universal gas constant, and T is temperature.

When using the ideal gas law equation, pressure should be in Pascals (Pa), volume in cubic meters (m³), and temperature in Kelvin (K).

The universal gas constant (R) is a value that accounts for the proportionality between the pressure, volume, and temperature of an ideal gas, always equaling 8.3 J K⁻¹ mol⁻¹.

The relative molecular mass of a substance is the mass of one molecule relative to 1/12th the mass of a carbon-12 atom. For a volatile liquid, it can be determined by experiment.