Kinetic Molecular Theory Trivia Quiz

The concept of an ideal gas is used to explain the behavior of a gas sample. The behavior of a gas sample refers to its properties, such as pressure, volume, and temperature, and how these properties are related to each other. The ideal gas law, which is based on the concept of an ideal gas, describes the relationship between these properties and allows us to predict and explain the behavior of gases under different conditions.

When the temperature of a gas sample is increased, the kinetic energy of the gas particles also increases. This causes the gas particles to move faster and collide more frequently with each other and the walls of the container. As a result, the gas sample behaves more like an ideal gas, where the gas particles are assumed to have negligible volume and no intermolecular forces.

On the other hand, when the pressure of a gas sample is decreased, the gas particles have more space to move around and collide with each other. This reduces the likelihood of intermolecular interactions and deviations from ideal gas behavior. Therefore, the combination of increased temperature and decreased pressure will cause the gas sample to behave more like an ideal gas.

The kinetic molecular theory assumes that the particles of an ideal gas are in random, constant, straight-line motion. This means that the particles move in a random manner, with no specific pattern or arrangement. They also move at a constant speed and in a straight line, until they collide with other particles or the walls of the container. This assumption helps explain the macroscopic properties of gases, such as pressure and temperature, based on the behavior of individual gas particles.

Oxygen gas behaves most like an ideal gas under high temperature and low pressure conditions. At high temperatures, the kinetic energy of the gas particles increases, causing them to move more rapidly and collide more frequently. This results in a more random and chaotic motion, which is a characteristic of an ideal gas. Additionally, at low pressures, the intermolecular forces between oxygen gas particles are weaker, allowing them to behave more like independent particles with negligible interactions.

At higher temperatures and lower pressures, a gas is more likely to behave like an ideal gas. In this case, 150°C and 100 kPa represent higher temperature and lower pressure compared to the other options, making it the best choice for the sample of H2(g) to behave most like an ideal gas.

At higher temperatures and lower pressures, gases tend to behave more like ideal gases. This is because at higher temperatures, the kinetic energy of the gas particles increases, causing them to move more rapidly and collide with each other less frequently. At lower pressures, the gas particles are more spread out, resulting in fewer intermolecular interactions. Therefore, the conditions of 750K and 20kPa would make helium behave most like an ideal gas.

To determine which gas sample has the same total number of molecules as 2.0 liters of CO22​ (g) at STP (Standard Temperature and Pressure), we need to apply Avogadro's Law. This law states that equal volumes of gases at the same temperature and pressure contain the same number of molecules.

Since the volume of the gas is directly proportional to the number of molecules, any gas at the same conditions (STP) having the same volume as another will contain the same number of molecules. This is irrespective of the chemical identity or molar mass of the gases.

Given:

2.0 liters of CO22​ at STP.

We are looking for another gas sample with the same volume at STP to have the same number of molecules. Among the options:

5.0 L of CO22​ (g) - This contains more than 2.0 L of CO22​ hence more molecules.

2.0 L of Cl22​ (g) - This contains the same volume as 2.0 L of CO22​ at STP, therefore, it has the same number of molecules.

3.0 L of H22​S (g) - This contains more than 2.0 L of CO22​ hence more molecules.

6.0 L of He (g) - This contains more than 2.0 L of CO22​ hence more molecules.

The correct answer is: 2.0 L of Cl22​ (g) - This sample has the same total number of molecules as 2.0 liters of CO22​ at STP.

When gas molecules are far apart and have weak attractive forces between them, they are able to move more freely and independently. This is similar to the behavior of ideal gases, which are assumed to have no intermolecular forces and occupy no volume. In contrast, when gas molecules are close together and have strong attractive forces between them, they are more likely to deviate from ideal gas behavior and exhibit properties such as condensation and liquefaction. Therefore, the statement suggests that a real gas behaves more like an ideal gas when the gas molecules are far apart and have weak attractive forces between them.

At higher temperatures and lower pressures, gases tend to behave more like ideal gases. This is because at higher temperatures, the kinetic energy of the gas particles increases, causing them to move faster and collide more frequently, resulting in a more random and uniform distribution of particles. At lower pressures, the intermolecular forces between the gas particles become less significant compared to the kinetic energy, allowing the gas particles to move more freely and independently. Therefore, at 400 K and 0.25 atm, the sample of neon is most likely to behave like an ideal gas.

The statement that describes the particles in a sample of an ideal gas according to the kinetic molecular theory is that the motion of the gas particles is random and straight-line. This means that the particles move in all directions with no preferred direction and they travel in straight lines until they collide with other particles or the walls of the container. This behavior is explained by the concept of kinetic energy and the assumption that gas particles are in constant motion.

According to the kinetic molecular theory, the particles of an ideal gas are separated by great distances, compared to their size. This means that the particles are not closely packed together, but rather spread out. This is because the particles in an ideal gas are in constant motion and move freely in all directions. The large distances between the particles allow them to move independently and collide with each other and the walls of the container. This is why gases are able to expand and fill the entire volume of their container.

At high temperature and low pressure, the intermolecular forces between the gas particles become significant and cannot be ignored. These forces cause the gas particles to deviate from ideal behavior, resulting in a decrease in the gas's resemblance to an ideal gas. As a result, the gas behaves least like an ideal gas under these conditions.