Gas Laws Practice Quiz Answer Key

Boyle's Law states that for a fixed amount of gas at a constant temperature, the pressure is inversely proportional to the volume. This means as the volume decreases, the pressure increases, and vice versa.

Charles's Law relates the volume of a gas to its temperature when pressure is held constant. Keeping the pressure constant allows the direct proportionality between volume and temperature (in Kelvin) to be observed.

Standard Temperature and Pressure (STP) conditions are defined as 273 K for temperature and 1 atm for pressure. This benchmark is used to provide a common basis for comparing gas volumes.

Avogadro's Law indicates that, under constant temperature and pressure, the volume of a gas is directly proportional to the number of moles. This means that increasing the number of gas particles will increase the volume proportionally.

In the ideal gas law, 'R' represents the universal gas constant, which provides the relationship between pressure, volume, temperature, and the number of moles. Its value depends on the units used, and it is essential for converting between these parameters.

According to Boyle's Law, the product of pressure and volume remains constant when temperature is fixed. When the volume is halved, the pressure must double in order to maintain this relationship.

Charles's Law states that the volume of a gas increases directly with its absolute temperature when pressure is constant. Thus, an increase in temperature leads to a proportional increase in volume.

Using Boyle's Law (P1V1 = P2V2), doubling the pressure results in halving the volume. Therefore, if the original volume is 4.5 L, the new volume under 2 atm pressure is 2.25 L.

The Ideal Gas Law assumes that gas molecules have negligible volume, experience no intermolecular forces, and collide elastically. Electrostatic attractions between molecules, however, are not part of the ideal behavior and only become relevant for real gases.

At a constant temperature, an increase in the kinetic energy of gas molecules results in more forceful and frequent collisions with the container walls, leading to an increase in pressure. This behavior is a core principle of the kinetic molecular theory.

Avogadro's Law states that at constant temperature and pressure, the volume of a gas is directly proportional to the number of moles. Therefore, an increase in moles will lead to an increase in volume.

STP conditions (0°C and 1 atm) are used to standardize measurements so that gases can be compared under a uniform set of circumstances. This consistency simplifies calculations and comparisons between different gas samples.

The combined gas law integrates Boyle's, Charles's, and Gay-Lussac's Laws into one expression, demonstrating that the ratio of the product of pressure and volume to the temperature (PV/T) remains constant for a given amount of gas. This constant ratio is useful when solving for unknown variables under changing conditions.

Dalton's Law of Partial Pressures states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each gas. Each gas in the mixture contributes independently to the total pressure.

Gay-Lussac's Law states that the pressure of a gas increases in direct proportion to its absolute temperature when the volume is constant. This makes it the appropriate model for predicting pressure changes in a constant-volume heating experiment.

Using the Ideal Gas Law (n = PV/RT) under constant pressure, an increase in volume and temperature changes the V/T ratio. Here, a 40% increase in volume coupled with a 20% increase in temperature leads to a net increase in the number of moles, indicating that additional gas must have entered the system.

According to Gay-Lussac's Law, which holds temperature and pressure in direct proportion at constant volume, the pressure increases by the same factor as the temperature increase. Raising the temperature from 300 K to 450 K (a 1.5-fold increase) results in the pressure rising from 3.0 atm to 4.5 atm.

At high pressures, the assumptions of the Ideal Gas Law begin to break down due to molecular volume and intermolecular attractions. The Van der Waals equation introduces correction factors for these deviations, making it more accurate for describing real gases.

According to Avogadro's Law, at constant temperature and pressure, the volume of a gas is directly proportional to the number of moles present. Therefore, doubling the amount of gas results in a doubling of the volume.

A higher measured pressure compared to the prediction of the Ideal Gas Law can indicate that the volume used in calculations is larger than the actual volume. Overestimating the container's volume leads to underestimating the predicted pressure, resulting in the observed discrepancy.