The Behavior Of Gases Chapter 14

The combined gas law allows calculations for situations where none of the variables—pressure, temperature, or volume—are constant. This means that the combined gas law can be used to analyze situations where the pressure, volume, and temperature of a gas are all changing.

When too much air is pumped into a tire, the pressure inside the tire increases. If the pressure exceeds the strength of the tire walls, it can cause the tire to rupture or burst.

When the temperature of a gas increases, the gas particles gain thermal energy. This causes them to move faster and have a higher average kinetic energy. As the particles move faster, they also collide with the walls of their container with more energy, resulting in greater pressure. Therefore, the given explanation accurately describes how gases behave when the temperature increases.

Automobile tires rely on the behavior of gases to operate properly. They are filled with air, which provides cushioning and support for the vehicle. Air compressors are used to fill the tires with the correct amount of air pressure. Air brakes in vehicles also rely on the behavior of gases. They use compressed air to activate the braking system, allowing the driver to slow down or stop the vehicle. Aerosol cans, such as those used for spray paint or air fresheners, rely on the behavior of gases to propel the contents out of the can when the nozzle is pressed.

The gas laws, including Boyle's law, Charles's law, and Gay-Lussac's law, describe the relationship between pressure, temperature, and volume of a gas. These laws state that if one of these quantities is held constant, the other two will vary in a predictable way. Therefore, a single mathematical expression involving pressure, temperature, and volume can represent the gas laws.

Absolute zero is the temperature at which the average kinetic energy of gas particles theoretically becomes zero. It is the lowest possible temperature that can be achieved, where all molecular motion ceases. At this point, the particles have no kinetic energy and are in their lowest possible energy state. It is a fundamental concept in thermodynamics and is used as a reference point for temperature scales such as Celsius and Kelvin.

This equation represents Gay-Lussac's law because it states that the volume is held constant (V1 = V2) while studying the relationship between pressure and temperature. According to Gay-Lussac's law, when the volume of a gas is held constant, the pressure and temperature are directly proportional. Therefore, as the temperature increases, the pressure of the gas will also increase.

The correct answer is the combined gas law. This is a mathematical equation that relates the pressure, volume, and temperature of a gas. It states that the product of the initial pressure and volume divided by the initial temperature is equal to the product of the final pressure and volume divided by the final temperature. This law is used to calculate the changes in these properties when a gas undergoes a change in conditions.

The given answer is correct because the three statements mentioned describe the basic assumptions of the kinetic theory of gases. According to the kinetic theory, gas particles are assumed to be so small in relation to the distances between them that their individual volumes can be considered insignificant. It also assumes that there are no attractive or repulsive forces between gas particles. Lastly, the kinetic theory states that gas particles are in constant random motion, traveling in independent straight paths until they collide with each other or other objects. These assumptions form the foundation of the kinetic theory and help explain the macroscopic properties of gases.

When a tire is pumped up with air, additional air particles are introduced into the tire. As a result, the number of particles inside the tire increases, leading to an increase in pressure. This is because the increase in the number of particles results in more frequent collisions with the walls of the tire, causing an increase in pressure. Therefore, the correct answer is that the pressure increases inside the tire when it is pumped up with air.

Diffusion is the process by which gas molecules move from areas of higher concentration to areas of lower concentration. This occurs due to the random motion of gas particles. As gas molecules are constantly moving and colliding with each other, they tend to spread out and fill the available space evenly. This movement from higher to lower concentration is the result of the natural tendency of gas particles to distribute themselves uniformly. Effusion, on the other hand, refers to the escape of gas molecules through a small opening.

The contribution of the pressure of each gas in a mixture to the total pressure is called the partial pressure exerted by that gas. This means that each gas in a mixture exerts its own pressure independent of the other gases present. The total pressure of the mixture is the sum of the partial pressures of each gas.

This equation represents Charles's law because it states that the pressure is held constant. Charles's law states that the volume of a gas is directly proportional to its temperature, as long as the pressure and amount of gas are held constant. Therefore, if the pressure is held constant in this equation, it implies that the volume and temperature are directly proportional to each other, which is a characteristic of Charles's law.

The average kinetic energy of gas particles and their Kelvin temperature are directly proportional because temperature is a measure of the average kinetic energy of the particles in a system. As the temperature increases, the average kinetic energy of the gas particles also increases. This relationship is described by the ideal gas law, which states that the product of pressure and volume is directly proportional to the absolute temperature of a gas. Therefore, an increase in temperature leads to an increase in the average kinetic energy of the gas particles.

The expression (P x V) / (T x n) represents the ideal gas law equation, where P is pressure, V is volume, T is temperature, and n is the number of moles of gas. According to the ideal gas law, for an ideal gas, the product of pressure and volume is directly proportional to the product of temperature and the number of moles of gas. This relationship holds true for all values of pressure, temperature, and volume under which the gas can exist. Therefore, the correct answer is an ideal gas.

The question asks for the name, symbol, and common unit for the variables used to describe the characteristics of a gas. The variables mentioned are pressure (P) measured in kilopascals, volume (V) measured in liters, temperature (T) measured in kelvins, and number of particles (n) measured in moles. This answer provides the correct information for describing the characteristics of a gas.

When the temperature of an enclosed gas is raised, the particles of the gas gain more kinetic energy and move faster. This increased motion leads to more frequent and forceful collisions with the walls of the container. As a result, the force exerted by the gas on the walls increases, causing an increase in pressure. Therefore, raising the temperature of an enclosed gas causes its pressure to increase.

The answer "true about ideal gases and the kinetic theory" is correct because it states that there is no real gas that exactly conforms to the kinetic theory and the ideal gas law. This is true because the kinetic theory assumes that gas particles are point masses with no volume, and that there are no intermolecular forces between them. In reality, gas particles do have volume and there are intermolecular forces present, although they may be negligible under certain conditions of temperature and pressure. Therefore, real gases behave very much like ideal gases under these conditions.

When a sealed bag of potato chips bulges near a sunny window, it suggests that the temperature inside the bag increases. According to the ideal gas law, an increase in temperature leads to an increase in the pressure exerted by the gas. This can be explained by the kinetic theory of gases, which states that as temperature increases, the average kinetic energy of gas molecules also increases. This increased kinetic energy causes the gas molecules to move faster and collide more frequently with the walls of the bag, resulting in an increase in pressure.

The fourth variable in the system is the amount of gas. This suggests that the system being referred to involves different states of matter, and the amount of gas present is one of the variables being considered.

Boyle's law states that for a given mass of gas at a constant temperature, the volume of the gas varies inversely with pressure. This means that as the pressure of a gas increases, its volume decreases, and vice versa, as long as the temperature remains constant. It is named after Robert Boyle, an Irish scientist who discovered this relationship in the 17th century.

When a sealed container of gas is opened, gas will flow from the region of higher pressure to the region of lower pressure. This is because gases tend to move from areas of high pressure to areas of low pressure in order to equalize the pressure. As the gas molecules are released from the container, they will naturally move towards the area where the pressure is lower, creating a flow from high pressure to low pressure.

Dalton's law of partial pressures states that at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases. This means that each gas in a mixture exerts its own pressure independently of the other gases present. The total pressure is simply the sum of these individual pressures. This law is based on the idea that gas molecules do not interact with each other and behave independently.

The correct answer is (P x V) / (n x R x T). This is because the ideal gas law, PV = nRT, states that the product of pressure (P) and volume (V) divided by the product of the number of moles (n), the ideal gas constant (R), and the temperature (T) always equals 1 for an ideal gas.

The gases used to inflate the airbag are compressible, meaning they can be compressed or squeezed into a smaller volume. This allows the airbag to absorb the energy from the impact by compressing the gas inside. As the gas is compressed, it absorbs the energy and helps to cushion the crash dummy, preventing it from being broken or injured.

When the spray button on an aerosol spray can is pressed, it creates an opening between the atmosphere and the gas inside the can. The gas inside the can is at a higher pressure, so it rushes out of the opening. This force pushes the product in the can and out with it, allowing it to be sprayed.

Gas pressure depends on the number of gas particles in a given volume and their average kinetic energy. The kinetic energy of the gas particles is directly related to their speed and motion. As the particles move faster and collide with the walls of the container more frequently, the pressure increases. The type of particle does not affect the gas pressure, as long as the number of particles and their average kinetic energy remain constant.

At a specified temperature and pressure, the number of moles of gas in a sample is directly proportional to the volume of the sample. This means that as the number of moles of gas increases, the volume of the sample also increases, and vice versa. This relationship is described by the ideal gas law, which states that the product of the number of moles and the volume of a gas is directly proportional to the temperature and pressure. Therefore, the correct answer is "directly proportional."

The correct answer is kinetic theory. The kinetic theory of gases assumes that gases consist of a large number of small particles that are in constant random motion. It also assumes that these particles have negligible volume and do not interact with each other except during collisions. This theory helps to explain various properties and behaviors of gases, such as their pressure, temperature, and volume relationships. Therefore, for a gas to meet the assumptions of the kinetic theory, it must behave in an "ideal" way.

A gas that follows the gas laws over a certain range of temperature and pressure is said to exhibit ideal behavior under those conditions. Ideal behavior refers to a gas that obeys the ideal gas law, which states that the pressure, volume, and temperature of a gas are related by a simple equation. In ideal behavior, the gas molecules do not interact with each other, and their volume is negligible compared to the volume of the container. This behavior is observed in real gases under low pressure and high temperature conditions.

Gay-Lussac's law states that the pressure of a gas is directly proportional to its temperature, when the volume is constant. This relationship can be expressed mathematically as P1/T1 = P2/T2, where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature. The temperatures in this equation must be measured on the Kelvin scale, as it is the only temperature scale that starts at absolute zero. Therefore, the correct answer is Kelvin's Scale.

Throwing aerosol cans into a fire is dangerous because it causes the gas pressure inside the can to increase greatly. The heat from the fire causes the propellant gas inside the can to expand rapidly, leading to a significant increase in pressure. This increased pressure can cause the can to burst and potentially explode, releasing the contents of the can in a violent manner. This can result in serious injuries or property damage due to flying debris or the release of flammable or toxic substances.

This equation represents Boyle's law because it states that when the temperature is held constant, the volume of a gas is inversely proportional to its pressure. In other words, as the pressure increases, the volume decreases, and vice versa.

The explanation for the correct answer, "compressibility of gases," is that the large relative distances between gas particles create empty space between them. This assumption of gas particles being far apart explains why gases are compressible. Compressibility refers to the measure of how much the volume of matter decreases under pressure.

Charles's law states that the volume of a gas is directly proportional to its temperature, assuming pressure and amount of gas remain constant. The equation for Charles's law is V1/T1 = V2/T2, where V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures. The temperatures in this equation must be measured on the Kelvin scale, as Kelvin is the absolute temperature scale where 0 Kelvin represents absolute zero. Therefore, the correct answer is Kelvin temperature.

At standard temperature and pressure (STP), one mole of any gas occupies a volume of 22.4 L. The given answer of 6.02 x 10^23 particles is consistent with Avogadro's number, which represents the number of particles (atoms, molecules, or ions) in one mole of a substance. Therefore, the correct answer is 6.02 x 10^23 particles, as one mole of gas particles occupies a volume of 22.4 L at STP.

The kinetic theory explains the behavior of gases with respect to conditions such as temperature and pressure. According to this theory, gases are composed of tiny particles that are in constant motion. The motion of these particles increases with higher temperatures, causing them to collide with each other and the walls of the container, resulting in pressure. Additionally, the kinetic theory explains how changes in temperature and pressure affect the volume, density, and other properties of gases.

As the nonzero volume of gas particles tends to increase, the overall volume of the gas also increases. When the volume increases, the numerator of the ratio (P x V) becomes larger, while the denominator (n x R x T) remains constant. Therefore, the ratio (P x V)/(n x R x T) becomes greater than 1, indicating an increase in volume.

The correct answer is Boyle's law. Boyle's law states that at constant temperature, the pressure of a gas is inversely proportional to its volume. In other words, as the volume of a gas decreases, the pressure increases, and vice versa. The statement in the question that "pressure times volume is constant" aligns with Boyle's law, as it demonstrates the inverse relationship between pressure and volume at constant temperature.

When two variables are directly proportional, it means that as one variable increases, the other variable also increases in such a way that the ratio between them remains constant. In other words, the two variables have a consistent relationship where their values change in sync, maintaining a fixed proportion between them. This can be visualized as a straight line on a graph, where an increase in one variable corresponds to a proportional increase in the other variable.

If two bodies have the same kinetic energy but different masses, it means that the body with the greater mass must be moving slower. This is because kinetic energy is directly proportional to the mass of an object, but inversely proportional to its velocity. Therefore, if the kinetic energy is the same, a greater mass will result in a slower velocity.

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The correct answer is "The number of moles must be constant, n1 lower = n 2 lower, for all three of these gas laws." This is because Boyle's law, Charles's law, and Gay-Lussac's law all involve the relationship between pressure, volume, and temperature of a gas. In each of these laws, the number of moles of the gas remains constant.

An inverse relationship occurs when one variable increases as the other decreases. This means that as one variable goes up, the other variable goes down. This is the opposite of a direct relationship, where both variables increase or decrease together. In an inverse relationship, there is a negative correlation between the two variables, indicating that they move in opposite directions.

The correct answer states that knowing the gas constant, R, and the ideal gas law equation, P x V = n x R x T, allows you to calculate the number of moles of gas at any specified values of pressure (P), volume (V), and temperature (T). This is because the ideal gas law relates these variables and the gas constant is a proportionality constant that allows for the conversion between different units of measurement. By rearranging the equation, you can solve for the number of moles (n) of gas.

This answer is correct because it accurately describes the relationship between volume and pressure in an enclosed gas held at constant temperature. According to Boyle's Law, when the pressure of a gas increases, the volume decreases, and when the pressure decreases, the volume increases. This inverse relationship between pressure and volume is a fundamental principle in gas laws.

The correct answer is "Gas particles are attracted to each other" and "Gas particles have some volume." In reality, gas particles do experience attractive forces between each other, especially at close distances. Additionally, gas particles do have a certain volume, although it is often considered negligible compared to the volume of the container they are in.

The reason Avogadro's hypothesis is reasonable is because it states that as long as the gas particles are not tightly packed, there is a significant amount of empty space between them. This means that a container can easily accommodate the same number of relatively large or relatively small gas particles. This hypothesis is based on the observation that gases can be compressed and expand to fill their container, indicating that the particles are not tightly packed together. Therefore, it is reasonable to assume that the size of the gas particles does not affect their ability to occupy the same volume of space.

The magnitude of the marked intervals on the pressure axis of the graph is 20,000 kPa. This means that each interval on the graph represents a pressure change of 20,000 kPa.

Avogadro's hypothesis states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. This means that regardless of the type of gas, if they are at the same temperature and pressure, they will have the same number of molecules. This hypothesis is important in understanding the behavior and properties of gases, as it allows us to make comparisons and calculations based on the volume and number of particles present.