Gas Laws and Properties Quiz

A property of gases where they expand to fill the entire volume of their container. Think of air filling a balloon.

A property of matter where substances mix together in any proportion. This is why we can have air, which is a mix of gases.

The force exerted by a gas on the walls of its container. Imagine air pushing on the inside of a tire.

The force exerted by the atmosphere on Earth's surface. It's the weight of the air above us.

A device used to measure atmospheric pressure. It measures the height of a mercury column to determine the pressure.

The force exerted by a gas on the surface of a liquid, measured using a device called a manometer.

PV = nRT, a law that describes the relationship between pressure (P), volume (V), moles (n), temperature (T), and a constant called the Ideal Gas Constant (R) for ideal gases.

The equation PV = nRT assumes that gas molecules have no volume and do not interact with each other. This is a theoretical concept used to simplify gas behavior calculations.

The mass of a substance per unit volume, often expressed in g/L for gases.

The upward force exerted on an object immersed in a fluid (gas or liquid), caused by the difference in pressure between the top and bottom of the object.

The relationship between gas density and temperature, stating that density decreases as temperature increases.

The volume occupied by one mole of a gas at standard temperature and pressure (STP).

The calculation of the amount of reactants and products involved in a chemical reaction, using the mole concept and balanced chemical equations.

A chemical reaction that involves the decomposition of sodium chlorate (NaClO3) with iron (Fe) to produce oxygen gas (O2) and solid sodium chloride (NaCl) plus iron oxide (FeO), commonly used in airplane oxygen generators.

The volume of a gas is dependent on pressure and temperature. This relationship can be expressed by the ideal gas law.

The number of moles of a substance is directly proportional to its mass and inversely proportional to its molar mass.

The stoichiometric coefficients in a balanced chemical equation represent the molar ratios of reactants and products.

A conversion factor linking moles of one substance to moles of another substance based on the stoichiometric coefficients in a balanced chemical equation.

A calculation that determines the amount of product that can be formed from a given amount of reactant, based on the stoichiometric relationships in a balanced chemical equation.

The amount of product actually obtained from a chemical reaction, which is often less than the theoretical yield due to factors like incomplete reactions or side reactions.

A gas's density is inversely proportional to its temperature. Higher temperatures = less dense gas.

The sum of the partial pressures of each gas within a mixture equals the total pressure.

The ratio of the number of moles of a component in a mixture to the total number of moles.

Pressure is proportional to the number of moles of gas. More moles = Higher pressure.

A gas collected over water contains both the target gas and water vapor.

A theory that explains the behavior of gases based on the movement and properties of gas molecules.

A gas law that describes the relationship between pressure and volume. Decreasing volume increase pressure.

A gas law that describes the relationship between volume and moles. More moles, more volume.

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

The ideal gas constant is a proportionality constant used in the ideal gas law. It relates the energy units to the units of temperature, volume, and pressure. Its value is 0.08206 L atm/(K mol).

The combination of Boyle's Law (PV = constant), Charles's Law (V/T = constant), and Avogadro's Law (V/n = constant) results in the ideal gas law. This means the ideal gas law encompasses the relationships between pressure, volume, temperature, and the number of moles.

STP is the standard temperature and pressure, a reference point for gas measurements. It is defined as 1 atm pressure and 273 K (0 °C) temperature.

Molar volume is the volume occupied by one mole of an ideal gas at STP. It is a constant value, approximately 22.4 L for most gases.

Gas stoichiometry involves using the mole ratios from balanced chemical equations to relate the amounts of reactants and/or products in gaseous reactions. The ideal gas law can be used to convert between moles of gas and its volume, pressure, and temperature.

Gases have no definite volume and expand to fill the container they are in. This is because gas molecules have a large amount of space between them and move freely.

The ideal gas model assumes that gas molecules have no volume and do not interact with each other. This is a simplification used to make calculations easier, but it is not completely accurate for real gases.