# The Behavior Of Gases Chapter 14

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Gases are all around us and they are all unique in their own way be it in behavior or location they are found. In chapter fourteen we got to understand the behavior of various gasses and their qualities. The quiz below is designed to test how well you understood that. Give it a try!

• 1.

### . What theory explains the behavior of gases with respect to conditions such astemperature and pressure?

• A.

Potential theory

• B.

Kinetic theory

• C.

Gas theory

B. Kinetic theory
Explanation
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.

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• 2.

### If you notice that a sealed bag of potato chips bulges when placed near a sunny window, what can you hypothesize about the relationship between the temperature and pressure of an enclosed gas?

• A.

An increase in temperature causes an increase in the pressure exerted by the gas.

• B.

An increase in temperature causes an decrease in the pressure exerted by the gas.

• C.

An decrease in temperature causes an increase in the pressure exerted by the gas.

A. An increase in temperature causes an increase in the pressure exerted by the gas.
Explanation
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.

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• 3.

### 1.Gas particles are so small in relation to the distances between them that their individual volumes can be assumed to be insignificant.2. No attractive or repulsive forces exist between gas particles.3.Gas particles are in constant random motion, traveling in independent straight paths until they collide with each other or other objects.

• A.

Three basic assumptions of the potenial theory about the properties of gases.

• B.

Three basic assumptions of the kinetic theory about the properties of gases.

• C.

Three basic assumptions of the gas theory about the properties of gases.

B. Three basic assumptions of the kinetic theory about the properties of gases.
Explanation
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.

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• 4.

### The large relative distances between gas particles means that there is considerable empty space between them.The assumption that gas particles are far apart explains gas compressibility.Compressibility is a measure of how much the volume of matter decreasesunder pressure.

• A.

Non compressibility of gases.

• B.

Compressibility of gases.

• C.

Gas particle compressibility

B. Compressibility of gases.
Explanation
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.

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• 5.

### Look at Figure 12.1 on page 327. How does an automobile air bag protect the crash dummy from being broken as a result of impact?

• A.

The gases used to inflate the airbag are compressible and are able to absorb a considerable amount of energy.

• B.

The gases used to inflate the airbag are not compressible and are able to absorb a considerable amount of energy.

• C.

The gases used to inflate the airbag are compressible and are not able to absorb a considerable amount of energy.

A. The gases used to inflate the airbag are compressible and are able to absorb a considerable amount of energy.
Explanation
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.

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• 6.

### . b. c. pressure, P. kilopascals volume, V, liters temperature, T, kelvins number of particles, n, moles

• A.

The name, the symbol, and a common unit for the four variables that are generally used to describe the characteristics of a liquids.

• B.

The name, the symbol, and a common unit for the four variables that are generally used to describe the characteristics of a gas.

• C.

The name, the symbol, and a common unit for the four variables that are generally used to describe the characteristics of a solids.

B. The name, the symbol, and a common unit for the four variables that are generally used to describe the characteristics of a gas.
Explanation
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.

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• 7.

### Four everyday items that rely on the behavior of gases to operate properly.

• A.

Feet, hands, legs,arms

• B.

Chair, table shoes,windows

• C.

Automobile tires,air compressors, air brakes,aerosol cans

C. Automobile tires,air compressors, air brakes,aerosol cans
Explanation
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.

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• 8.

### How do conditions change inside a tire when you pump it up with a tirenumn?

• A.

Because air particles are added, the pressure increases inside the tire.

• B.

Because air particles are added, the pressure decreases inside the tire.

• C.

Because air particles are taken away, the pressure increases inside the tire.

A. Because air particles are added, the pressure increases inside the tire.
Explanation
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.

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• 9.

### What can happen if too much air is pumped into a tire?

• A.

The pressure inside the tire can increase beyond the strength of its walls, causing the tire to rupture or burst.

• B.

The pressure inside the tire can decrease beyond the strength of its walls, causing the tire to rupture or burst.

• C.

The pressure outside the tire can decrease beyond the strength of its walls, causing the tire to rupture or burst.

A. The pressure inside the tire can increase beyond the strength of its walls, causing the tire to rupture or burst.
Explanation
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.

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• 10.

### When a sealed container of gas is opened, gas will flowfrom the region of higher pressure to the region of__________ pressure.

• A.

Same

• B.

Higher

• C.

Lower

C. Lower
Explanation
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.

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• 11.

### Pushing the button creates an opening between the atmosphere and the gas inside the can, which is at a higher pressure.Gas from inside the can rushes out of the opening, forcing the product in the can and out with it.

• A.

The jar of pickles will closs tightly.

• B.

The garbage can lid will pop off.

• C.

The spray button on an aerosol spray can is pressed.

C. The spray button on an aerosol spray can is pressed.
Explanation
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.

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• 12.

### Raising the temperature of an enclosed gas causes its pressure to ___________.

• A.

Increase

• B.

Decrease

• C.

Stay the same

A. Increase
Explanation
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.

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• 13.

### The average kinetic energy of the gas particles increases as the particles absorb thermal energy.Faster-moving particles impact the walls of their container with more energy, exerting greater pressure.

• A.

Describes how gases behave when the temperature increases

• B.

Describes how gases behave when the temperature decreases

• C.

Describes how gases behave when the temperature istays the same

A. Describes how gases behave when the temperature increases
Explanation
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.

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• 14.

### Throwing an aerosol can into a fire causes the gas pressure inside the can to increase greatly, with the likelihood that the can will burst.

• A.

Explain why it is dangerous to bounce an aerosol can into a fire.

• B.

Explain why it is dangerous to open aerosol cans over a fire.

• C.

Explain why it is dangerous to throw aerosol cans into a fire.

C. Explain why it is dangerous to throw aerosol cans into a fire.
Explanation
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.

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• 15.

### What is Daltoris law of partial pressures?

• A.

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.

• B.

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 liquid.

• C.

At constant volume and temperature, the total non pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.

A. 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.
Explanation
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.

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• 16.

### The tendency of gas molecules to move from areas of higher concentration toareas of lower concentration is called

• A.

Gases

• B.

Diffusion

• C.

Effusion

B. Diffusion
Explanation
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.

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• 17.

### If two bodies with different masses have the same kinetic energy, the one with the greater mass must move __________.

• A.

The same

• B.

Slower

• C.

Faster

B. Slower
Explanation
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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• 18.

### Which of the gases shown has behavior that is close to ideal ranging from near0 kPa to almost 40 000 kPa?

• A.

CH 4 exponent at 100 °C

• B.

CH 4 exponent at 300 °C

• C.

CH 4 exponent at 200 °C

C. CH 4 exponent at 200 °C
• 19.

### Two assumptions of simple kinetic theory that are incorrect for real gases?

• A.

Gas particles are attracted to each other. k Gas particles have some volume.

• B.

Gas particles are not attracted to each other. k Gas particles have no volume.

• C.

Gas particles are attracted to each other. k Gas particles have alot volume.

B. Gas particles are not attracted to each other. k Gas particles have no volume.
Explanation
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.

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• 20.

### The nonzero volume of gas particles tends to __________volume, making the ratio (P x V)/(n x R x T) greater than 1.

• A.

Increase

• B.

Decrease

• C.

Stays the same

A. Increase
Explanation
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.

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• 21.

### _______________ says that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.

• A.

Boyle's hypothesis

• B.

Charles hypothesis

• C.

Explanation
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.

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• 22.

### Why is Avogadro's hypothesis reasonable?

• A.

As long as the gas particles are not tightly packed, there is a great deal of occupied space between them, A container can easily accommodate the same number of relatively large or relatively small gas particles.

• B.

As long as the gas particles are not tightly packed, there is a great deal of empty space between them, A container can easily accommodate the same number of relatively large or relatively small gas particles.

• C.

As long as the gas particles are not tightly packed, there is a great deal of occupied space between them, A container can easily accommodate the same number of relatively large or relatively large gas particles.

B. As long as the gas particles are not tightly packed, there is a great deal of empty space between them, A container can easily accommodate the same number of relatively large or relatively small gas particles.
Explanation
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.

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• 23.

### How many gas particles occupy a volume of 22.4 L at standard temperature and pressure?

• A.

6.02 x 1Q 30 exponents particles

• B.

6.02 x 1Q 25 exponents particles

• C.

6.02 x 1Q 23 exponents particles

C. 6.02 x 1Q 23 exponents particles
Explanation
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.

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• 24.

### Gas pressure depends only on thenumber of gas particles in a given volume and on their average ________—the type of particle does not matter.

• A.

Gas energy

• B.

Potential energy

• C.

Kenetic energy

C. Kenetic energy
Explanation
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.

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• 25.

### 4.      The contribution of the pressure of each gas in a mixture to the total pressure is called the _________ exerted by that gas.

• A.

Partial pressure

• B.

Complete pressure

• C.

No pressure

A. Partial pressure
Explanation
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.

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• 26.

### To meet the assumptions of___________of gases, gases must behave in an "ideal" way.

• A.

Potential theory

• B.

Kinetic theory

• C.

Gas theory

B. Kinetic theory
Explanation
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.

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• 27.

### There is no real gas that exactly conforms to the kinetic theory and the ideal gas law.At many conditions of temperature and pressure, real gases behave very much like ideal gases.

• A.

True about ideal gases and the potential theory.

• B.

True about ideal gases and the kinetic theory.

• C.

True about ideal gases and the gas theory.

B. True about ideal gases and the kinetic theory.
Explanation
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.

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• 28.

### If a gas were truly an ideal gas, it would be _________to liquefy or solidify it by cooling or by applying pressure.

• A.

Important

• B.

Possible

• C.

Impossible

C. Impossible
Explanation
If a gas were truly an ideal gas, it would be impossible to liquefy or solidify it by cooling or by applying pressure. This is because an ideal gas is a theoretical concept that assumes no intermolecular forces or volume for the gas particles. In reality, gases have intermolecular forces that become significant at low temperatures or high pressures, causing them to condense into liquids or solids. Therefore, it is impossible to achieve liquefaction or solidification of a gas if it behaves as an ideal gas.

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• 29.

### 15.  A gas that follows the gas laws over a certain range of temperature and pressure is said to exhibit____________ under those conditions.

• A.

Less than ideal behavior

• B.

Ideal behavior

• C.

No behavior

B. Ideal behavior
Explanation
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.

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• 30.

### What ratio always equals 1 for an ideal gas?

• A.

___(P x V)____ (n x R x T)

• B.

___(P x V)____ (n R x T)

• C.

__2_(P x V)____ (n x R x T)

A. ___(P x V)____ (n x R x T)
Explanation
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.

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• 31.

### What is the magnitude of the marked intervals on the pressure axis of the graph?.

• A.

30 000 kPa

• B.

20 000 kPa

• C.

10 000 kPa

B. 20 000 kPa
Explanation
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.

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• 32.

### Which of the gases shown deviates the most from ideal at pressures less than 20 000 kPa?

• A.

CO 8 exponent at 40 °C

• B.

CO 4 exponent at 40 °C

• C.

CO 2 exponent at 40 °C

C. CO 2 exponent at 40 °C
Explanation
CO2 deviates the most from ideal at pressures less than 20 000 kPa because it has the highest exponent value compared to the other gases. This indicates that CO2 has a larger deviation from ideal gas behavior, meaning it is less likely to follow the ideal gas law at low pressures.

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• 33.

### At a specified temperature and pressure, is the number of moles of gas in a sample directly proportional or inversely proportional to the volume of the sample?

• A.

Not directly proportional

• B.

Directly proportional

• C.

Indirectly proportional

B. Directly proportional
Explanation
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."

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• 34.

### The correct description of how the combined gas law must be modified when you measure the amount of a gas in moles.

• A.

Multiply each side of the equation by the number of moles.

• B.

Divide each side of the equation by the number of moles.

• C.

Add the number of moles to each side of the equation.

B. Divide each side of the equation by the number of moles.
Explanation
When measuring the amount of a gas in moles, the combined gas law equation needs to be modified by dividing each side of the equation by the number of moles. This is because the number of moles represents the quantity of gas, and dividing by this value allows us to isolate the other variables in the equation and calculate their values.

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• 35.

### For what kind of gas is (P x V) I (T x n} a constant for all values of pressure,temperature, and volume under which the gas can exist?

• A.

An ideal volumn

• B.

An ideal mass

• C.

An ideal gas

C. An ideal gas
Explanation
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.

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• 36.

### Which variable in the equation (Pi x VJ = (P2 x ^2) CT, x nj     (Z*2 x n2) is constant in Boyle's law, Charles's law, and Gay-Lussac's law?

• A.

The number of moles must be constant, n1 lower = n 2 lower , for all three of these gas laws.

• B.

The number of moles must be constant, n2 lower = n 2 lower , for all three of these gas laws.

• C.

The number of moles must be constant, n1 lower = n 3 lower , for all three of these gas laws.

A. The number of moles must be constant, n1 lower = n 2 lower , for all three of these gas laws.
Explanation
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.

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• 37.

### Why would you use the ideal gas law when you know the gas constant instead of the combined gas law?

• A.

Knowing the gas constant, T, and the ideal gas Saw, P x V = n x R x T lets you calculate the number of motes of gas at any specified values of P, V, and T.

• B.

Knowing the gas constant, R, and the ideal gas Saw, P x V = n x R x T lets you calculate the number of motes of gas at any specified values of P, V, and T.

• C.

Knowing the gas constant, n, and the ideal gas Saw, P x V = n x R x T lets you calculate the number of motes of gas at any specified values of P, V, and T.

B. Knowing the gas constant, R, and the ideal gas Saw, P x V = n x R x T lets you calculate the number of motes of gas at any specified values of P, V, and T.
Explanation
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.

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• 38.

### A single mathematical expression involving pressure, temperature, and volume can represent the _______of Boyle, Charles, and Gay-Lussac if one or another of these quantities is held constant.

• A.

Gas laws

• B.

Liquid laws

• C.

Solid laws

A. Gas laws
Explanation
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.

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• 39.

### The fourth variable is the amount of ___________ in the system.

• A.

Solid

• B.

Liquid

• C.

Gas

C. Gas
Explanation
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.

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• 40.

### What is this mathematical equation called?

• A.

The combined solid law

• B.

The combined liquid law

• C.

The combined gas law

C. The combined gas law
Explanation
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.

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• 41.

### 17.     Which gas law does this equation represent if temperature is held constant sothat T 2 lower T 2 lower ?

• A.

Boy|e's law

• B.

Charles's law

• C.

Gay-Lussac's law

A. Boy|e's law
Explanation
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.

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• 42.

### Which gas law does this equation represent if pressure is held constant so thatP 1 lower = P2 lower ?

• A.

Boy|e's law

• B.

Charles's law

• C.

Gay-Lussac's law

B. Charles's law
Explanation
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.

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• 43.

### Which gas law does this equation represent if volume is held constant so thatV 1 lower = V2 lower?

• A.

Boy|e's law

• B.

Charles's law

• C.

Gay-Lussac's law

C. Gay-Lussac's law
Explanation
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.

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• 44.

### The combined gas law allows calculations for situations where none of the variables—pressure, _____________, or volume—are constant.

• A.

Temperature

• B.

Liquid

• C.

Solid

A. Temperature
Explanation
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.

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• 45.

### What do you notice about the product of pressure times volume at constant temperature? What gas law does thisillustrate?

• A.

Pressure times volume is constant. This relationship illustratesGay-Lussac's law .

• B.

Pressure times volume is constant. This relationship illustrates Charles's law.

• C.

Pressure times volume is constant. This relationship illustrates Boyle's law.

C. Pressure times volume is constant. This relationship illustrates Boyle's law.
Explanation
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.

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• 46.

### The temperature at which average kinetic energy of gas particles theoreticallyis zero is called

• A.

Negative one

• B.

Absolute zero

• C.

zero

B. Absolute zero
Explanation
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.

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• 47.

### What does it mean to say that two variables are directly proportional?

• A.

When one variable decrease, the other increases so that the ratio of the two variables remains constant.

• B.

When one variable increases, the other increases so that the ratio of the two variables remains constant.

• C.

When one variable increases, the other increases so that the amount of the two variables remains constant.

B. When one variable increases, the other increases so that the ratio of the two variables remains constant.
Explanation
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.

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• 48.

### Charles's law states that when thepressure of a fixed _______of gas is held constant, the volume of the gas isdirectly proportional to its Kelvin temperature.

• A.

Mass

• B.

Volumn

• C.

Circumference

A. Mass
• 49.

### . Charles's law may be written  ___V1__ lower   =  __V2__  lower  temperatures are                                                      T1                         T2measured on what scale?.

• A.

Boyle temperatue

• B.

Kelvin temperature

• C.

Chsrles temperature

B. Kelvin temperature
Explanation
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.

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• 50.

### P         P 14.  Gay-Lussac's law may be written —~ = —f if the volume is constant and if the T1              T   2temperatures are measured on what scale?

• A.

Boyle's Scale

• B.

Kelvin's Scale

• C.

Gay's Scale

B. Kelvin's Scale
Explanation
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.

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• Mar 22, 2023
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• Mar 27, 2011
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