Gas Laws and Charles's Law Quiz

A law stating that the volume of a gas increases or decreases by 1/273 of its initial volume at 0°C for every 1°C rise or fall in temperature, keeping the pressure constant.

The temperature at which the volume of an ideal gas theoretically becomes zero. It is equal to -273°C or 0 Kelvin.

The relationship between volume and temperature of a gas, expressed as V₁/T₁ = V₂/T₂, where V₁ and V₂ are the initial and final volumes, and T₁ and T₂ are the initial and final absolute temperatures.

The volume of a given mass of a gas is directly proportional to its absolute temperature when pressure remains constant.

A graph that plots the volume of a gas against its temperature at constant pressure. The plot results in a straight line, and extrapolation of this line intersects the temperature axis at -273°C (absolute zero).

A gas law combining Boyle’s Law and Charles’s Law, demonstrating the simultaneous effect of pressure and temperature on volume.

The relationship between pressure, volume, and temperature of a gas, expressed as P₁V₁/T₁ = P₂V₂/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.

A gas equation that establishes the relationship between the volume of a gas and its absolute temperature. It can be written as V = constant × T.

The SI unit for molar gas constant (R) is mole^-1 K^-1.

The ideal gas law describes the relationship between pressure (P), volume (V), temperature (T), and the number of moles (n) of an ideal gas. It is represented by the equation: PV = nRT, where R is the molar gas constant.

The pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. This means that the total pressure is the sum of the pressures that each gas would exert if it were alone in the container.

NTP stands for Normal Temperature and Pressure. It is a standard set of conditions used to compare the properties of gases.

The standard temperature and pressure (STP) are widely used as a reference point for comparing the properties of gases. It is defined as a temperature of 0°C (273.15 K) and a pressure of 1 atmosphere (atm).

The volume of one mole of any gas at STP (standard temperature and pressure) is 22.4 liters. This is called the molar volume of an ideal gas.

A fire extinguisher uses the pressure created by a compressed gas to expel the extinguishing agent, which cools the fire and displaces the oxygen, preventing further combustion.

Describes the relationship between the pressure and volume of a fixed amount of gas at a constant temperature. As the volume of the gas decreases, the pressure increases proportionally.

A hypothetical gas that perfectly obeys all gas laws at all temperatures and pressures. Ideal gases do not exist in reality, but many real gases behave like ideal gases at low pressures and high temperatures.

A gas that does not perfectly obey the gas laws, especially under high pressure or low temperature conditions. Real gases have intermolecular forces and particle volume, affecting their behavior at certain conditions.

An equation that relates the pressure, volume, temperature, and number of moles of an ideal gas. It is a mathematical representation of the ideal gas law, a fundamental concept in chemistry and physics.

A constant that relates the pressure, volume, temperature, and number of moles of an ideal gas. Essentially, it is the constant of proportionality in the ideal gas law equation.

The conditions of standard pressure and temperature. Standard pressure is 1 atmosphere (atm), and standard temperature is 273 Kelvin (0 degrees Celsius).

The process of converting a liquid to a gas.

The mass of one mole of a substance, expressed in grams per mole (g/mol).

The amount of substance that contains as many elementary entities as there are atoms in 0.012 kilogram of carbon-12. It's approximately 6.022 x 10²³ entities.

A measure of the force exerted per unit area. It's often expressed in units of atmospheres (atm), millimeters of mercury (mmHg), or pascals (Pa).

The space occupied by a substance. It's typically measured in units like liters (L) or cubic meters (m³).

The pressure exerted by a single gas in a mixture of gases.

The sum of the partial pressures of each component gas in the mixture.

The volume occupied by one mole of a gas at standard temperature and pressure (STP), which is 22.4 liters at 0°C and 1 atmosphere.