Gas Laws Quiz - Chemistry Class

The force applied perpendicularly to a surface per unit area. Think of the difference in pressure when standing on your toes compared to standing with your entire foot flat on the ground.

The SI unit of pressure, equivalent to 1000 Newtons per square meter. It is commonly used for measuring gas pressures.

The standard ambient temperature and pressure, where the temperature is 25 degrees Celsius and the pressure is 100 kPa.

The standard temperature and pressure, where the temperature is 0 degrees Celsius and the pressure is 1 atmosphere (101.325 kPa).

The absolute zero point on the Kelvin scale, where the temperature is theoretically 0 Kelvin (or -273.15 degrees Celsius). At this temperature, all molecular motion ceases.

A relationship between pressure and volume where the product of pressure and volume remains constant at a constant temperature.

The temperature at which all molecular motion theoretically ceases, equivalent to 0 Kelvin (-273.15 °C).

The volume of a gas is directly proportional to its absolute temperature, assuming pressure and the number of moles of gas remain constant.

A combined gas law that describes the relationship between pressure, volume, and temperature of a fixed amount of gas.

The average kinetic energy of gas molecules is directly proportional to its absolute temperature. As temperature increases, molecules move faster and collide more frequently.

The force per unit area exerted by gas molecules colliding with the walls of their container. It's influenced by the frequency and force of collisions.

The direct relationship between the volume of a gas and its temperature, where the volume increases proportionally to the absolute temperature.

The weak forces of attraction between molecules that are relatively far apart in a gas.

Gases always expand to fill the container they are in, regardless of their shape or volume. Think of air filling up an empty balloon!

The volume of a gas can be decreased by applying pressure. Think of squeezing a balloon - the pressure inside increases and the volume decreases.

Changes in temperature affect the pressure and volume of a gas. Imagine heating up a balloon - it expands! Cool it down, and it shrinks!

P1V1 = P2V2 is the formula for Boyle's Law. It lets you calculate the pressure or volume of a gas if the other factor changes. Think of it like balancing a seesaw!

For Charles' Law, temperature is measured in Kelvin, not Celsius. Think of adding 273.15 to Celsius to convert to Kelvin!

A graph of Boyle's Law will show an inverse relationship between pressure and volume, where the curve goes down as pressure increases. Think of a seesaw!

Equal volumes of gases (at the same temperature and pressure) contain the same number of molecules, regardless of their chemical identity.

The volume of one mole of a gas at standard temperature and pressure (STP). At STP (0°C and 1 atm), the molar volume of a gas is approximately 22.7 L/mol.

The volume of one mole of a gas at standard ambient temperature and pressure (SATP). At SATP (25°C and 100 kPa), the molar volume of a gas is approximately 24.8 L/mol.

The relationship between the pressure and temperature of a fixed amount of gas at constant volume. The pressure of a gas is directly proportional to its absolute temperature.

A hypothetical gas that obeys all gas laws perfectly under all conditions. It doesn't condense into liquids, even at high pressures or low temperatures.

Real gases deviate most from ideal behaviour at high pressures and low temperatures. This is related to the Kinetic Molecular Theory, which describes how gas molecules move and interact.

Boyle's Law states that the volume of a gas is inversely proportional to its pressure, assuming the temperature and number of moles of gas remain constant. This means that as pressure increases, volume decreases, and vice versa.

Charles's Law states that the volume of a gas is directly proportional to its temperature, assuming the pressure and number of moles of gas remain constant. This means that as temperature increases, volume increases, and vice versa.

The combined gas law combines Boyle's and Charles's Law, showing the relationship between pressure, volume, and temperature of a gas when the number of moles remains constant. It states that the product of pressure and volume divided by temperature is constant.

The ideal gas law describes the relationship between pressure, volume, temperature, and the number of moles of an ideal gas. It states that the product of pressure and volume is equal to the product of the number of moles, the ideal gas constant, and the temperature.

The Law of Combining Volumes states that, under the same conditions of temperature and pressure, the volumes of reacting gases and their gaseous products are in simple whole number ratios. This law is based on the idea that the volume of a gas is directly proportional to the number of moles of gas present.

The universal gas constant (R) is a proportionality constant used in the Ideal Gas Law equation. It relates the pressure, volume, temperature, and number of moles of an ideal gas. Its value depends on the units used for pressure, volume, and temperature.

The molar mass of a substance is the mass of one mole of that substance. It's expressed in grams per mole (g/mol).

Percent difference is a way to quantify the relative difference between two values. It's calculated as the absolute difference between the two values divided by their average, multiplied by 100%.

Density is a measure of how much mass is contained in a given volume. It's expressed in units of mass per unit volume, such as grams per milliliter (g/mL) or kilograms per cubic meter (kg/m³).

Gas stoichiometry involves the study of the quantitative relationships between reactants and products in chemical reactions involving gases.

A balanced chemical equation represents a chemical reaction with equal numbers of atoms of each element on both the reactant and product sides. Balancing equations ensures that the law of conservation of mass is obeyed.

Mole ratio is the ratio of the number of moles of one substance to the number of moles of another substance in a balanced chemical equation. Mole ratios are used to convert between different quantities in chemical reactions.