Kinetic Theory and Gas Laws Quiz

<p>Torr (A)</p> Signup and view all the answers

<p>1000 L (A)</p> Signup and view all the answers

<p>Volume increases. (D)</p> Signup and view all the answers

<p>212 K (D)</p> Signup and view all the answers

<p>Pressure is directly proportional to temperature. (C)</p> Signup and view all the answers

<p>30.98 °C (D)</p> Signup and view all the answers

<p>Van der Waals equation (B)</p> Signup and view all the answers

<p>Liquefaction (A)</p> Signup and view all the answers

<p>73 atm (C)</p> Signup and view all the answers

<p>The pressure needed to liquefy a gas at its critical temperature (C)</p> Signup and view all the answers

<p>Increasing pressure (A)</p> Signup and view all the answers

<p>Volume occupied by one mole of gas at critical temperature and pressure (A)</p> Signup and view all the answers

<p>PV = nRT (A)</p> Signup and view all the answers

<p>Ideal behavior (A)</p> Signup and view all the answers

<p>Pressure decreases. (A)</p> Signup and view all the answers

<p>Low pressures and high temperatures (D)</p> Signup and view all the answers

<p>Gases behave ideally (D)</p> Signup and view all the answers

<p>Divide by 760. (A)</p> Signup and view all the answers

<p>Molecule volume should be subtracted from container volume (A)</p> Signup and view all the answers

<p>Due to attractions decreasing collision frequency (B)</p> Signup and view all the answers

<p>It can only be less than the ideal pressure (A)</p> Signup and view all the answers

<p>Volume doubles. (A)</p> Signup and view all the answers

<p>Available volume = V - nb (A)</p> Signup and view all the answers

<p>Total pressure is the sum of individual partial pressures. (D)</p> Signup and view all the answers

<p>Significantly increases attraction forces (C)</p> Signup and view all the answers

<p>20.18 g/mol (D)</p> Signup and view all the answers

<p>Charles' Law. (A)</p> Signup and view all the answers

<p>54.5 g/L (B)</p> Signup and view all the answers

<p>Both attraction and repulsion forces are operational (D)</p> Signup and view all the answers

<p>The ratio of the number of moles of the gas to the total number of moles of all gases present (C)</p> Signup and view all the answers

<p>It is the mole fraction of the gas multiplied by the total pressure. (C)</p> Signup and view all the answers

<p>The pressure will be five times higher. (A)</p> Signup and view all the answers

<p>It contains the same number of molecules as the carbon dioxide sample. (C)</p> Signup and view all the answers

<p>Diffusion rates are inversely proportional to the molar masses. (D)</p> Signup and view all the answers

<p>It is directly proportional to the molar mass of the gas. (D)</p> Signup and view all the answers

<p>55.0 minutes (C)</p> Signup and view all the answers

<p>0.0181 atm (D)</p> Signup and view all the answers

<p>76.4 g/mole (B)</p> Signup and view all the answers

<p>Higher temperatures and low pressures (A)</p> Signup and view all the answers

<p>Z &lt; 1 means volume is less than expected (A)</p> Signup and view all the answers

<p>Repulsive forces dominate over attractive forces (B)</p> Signup and view all the answers

<p>They do not coincide in certain cases (B)</p> Signup and view all the answers

<p>Attractive forces are initially dominant, then repulsive forces prevail (C)</p> Signup and view all the answers

<p>NH3, CO2, SO2 (C)</p> Signup and view all the answers

<p>PV equals the product of pressure and volume (B)</p> Signup and view all the answers

The state of matter characterized by widely separated molecules in rapid motion.

A substance that is typically found in the gaseous state at room temperature (25°C) and standard atmospheric pressure.

The force exerted per unit area by a gas on the walls of its container.

The volume of a gas is inversely proportional to its pressure at constant temperature and number of moles.

The volume of a gas is directly proportional to its absolute temperature at constant pressure.

The pressure of a gas is directly proportional to its absolute temperature at constant volume.

The combination of Boyle's Law, Charles's Law, and Gay-Lussac's Law. It states that the product of pressure and volume is proportional to the absolute temperature for a given amount of gas.

The pressure of a gas mixture is equal to the sum of the partial pressures of the individual gases in the mixture.

A relationship between the pressure, volume, temperature, and number of moles of a gas. It states that the product of pressure and volume is directly proportional to the product of the number of moles and the temperature.

The pressure of a gas is inversely proportional to its volume when the temperature and the amount of gas are held constant.

The volume of a gas is directly proportional to its absolute temperature when the pressure and the amount of gas are held constant.

The volume of a gas is directly proportional to the number of moles of gas when the temperature and the pressure are held constant.

The pressure of a gas is directly proportional to its absolute temperature when the volume and the amount of gas are held constant.

The total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases.

A measure of the mass of a substance per unit volume.

The mass of one mole of a substance.

The ratio of the number of moles of a specific gas to the total number of moles of gases present in a mixture.

The pressure exerted by a specific gas in a mixture.

The rate at which gas molecules diffuse through a porous barrier is inversely proportional to the square root of its molar mass.

The process by which a gas escapes from a container through a small opening.

The gradual mixing of gas molecules due to their random motion.

The average distance a gas molecule travels before colliding with another molecule.

A measure of how much a real gas deviates from ideal gas behavior.

When the compressibility factor (Z) is greater than 1, the real gas volume is larger than the ideal gas volume. This indicates repulsive forces dominate.

When the compressibility factor (Z) is less than 1, the real gas volume is smaller than the ideal gas volume. This indicates attractive forces dominate.

Permanent gases, like Helium and Hydrogen, are often associated with Z > 1. This means repulsive forces dominate.

Gases like Ammonia (NH3), Carbon Dioxide (CO2), and Sulfur Dioxide (SO2) are often associated with Z < 1, indicating attractive forces are more significant.

For gases like Helium and Hydrogen, the compressibility factor (Z) increases with increasing pressure, meaning repulsive forces become more dominant.

For gases like Methane (CH4), Carbon Dioxide (CO2), and Ammonia (NH3), the compressibility factor (Z) initially decreases with increasing pressure, indicating attractive forces dominate, but then increases at higher pressures, indicating repulsive forces become more dominant.

The isotherms of real gases deviate from the ideal gas behavior, showing that the actual volume of a real gas can be different from the theoretical ideal gas volume.

The pressure exerted by an ideal gas, calculated using the ideal gas law.

The pressure exerted by a real gas, taking into account the attractive and repulsive forces between gas molecules.

A mathematical equation used to predict the behavior of real gases, accounting for intermolecular forces and the volume occupied by gas molecules.

The temperature above which a gas cannot be liquefied, no matter how much pressure is applied.

The pressure required to liquefy a gas at its critical temperature.

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

The process of converting a gas into a liquid state. It can be achieved by cooling or pressurizing the gas.

Isotherms that show deviations from ideality at lower temperatures, indicating that real gases become non-ideal at lower temperatures.

The point on an isotherm where a gas begins to liquefy.

The steeply rising portion of an isotherm representing the liquid phase, where small volume changes cause large pressure increases.

The deviation from ideal behavior in real gases is due to the interplay of attractive and repulsive forces between gas molecules. At low pressures, attraction dominates, leading to lower pressure than ideal. At high pressures, repulsion becomes significant, causing a higher pressure than ideal.

As the pressure of a gas increases, the molecules get closer together. This increases the importance of the repulsive forces between them, leading to a larger deviation from ideal behavior.

At higher temperatures, gas molecules have more kinetic energy and move faster, weakening the attractive forces between them. This leads to a smaller deviation from ideal behavior.

The volume available for gas molecules is less than the container's volume, taking into account the space occupied by the molecules. This volume correction, nb, where 'b' is a constant specific to the gas, is subtracted from the container's volume.

The pressure exerted by a real gas is less than the ideal pressure due to the attractive forces between molecules, which reduce the frequency and impact of collisions with the container walls.

The reduction in pressure due to attractive forces is proportional to the square of the molar concentration (n/V) because more molecules in a smaller space lead to stronger interactions.