# Gas laws chemistry regents questions and answers

Created in the early 17th century, the gas laws have been around to assist scientists in finding volumes, amount, pressures and temperature when coming to matters of gas. The three fundamental gas laws discover the relationship of pressure, temperature, volume and amount of gas. Boyle's Law tells us that the volume of gas increases as the pressure decreases.

Charles' Law tells us that the volume of gas increases as the temperature increases. And Avogadro's Law tell us that the volume of gas increases as the amount of gas increases. The ideal gas law is the combination of the three simple gas laws. Ideal gas, or perfect gas, is the theoretical substance that helps establish the relationship of four gas variables, p ressure Pvolume Vthe amount of gas n and temperature T.

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It has characters described as follow:. Real gas, in contrast, has real volume and the collision of the particles is not elastic, because there are attractive forces between particles. As a result, the volume of real gas is much larger than of the ideal gas, and the pressure of real gas is lower than of ideal gas. All real gases tend to perform ideal gas behavior at low pressure and relatively high temperature. The compressiblity factor Z tells us how much the real gases differ from ideal gas behavior.

Another form of the equation assuming there are 2 sets of conditions, and setting both constants to eachother that might help solve problems is:. What will be the volume if the pressure becomes 1. Volume is directly proportional to Temperature. A sample of Carbon dioxide in a pump has volume of When the amount of gas and pressure remain constant, find the new volume of Carbon dioxide in the pump if temperature is increased to What will be the new volume of oxygen gas in the pump if temperature and pressure held constant?

By setting all three laws directly or inversely proportional to Volume, you get:.

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Next replacing the directly proportional to sign with a constant R you get:. Here, R is the called the gas constant. The value of R is determined by experimental results. Its numerical value changes with units. At mm Hg and How many moles of Chlorine gas at this condition?My Ad Code. Standard temperature is equal to.

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Standard pressure is equal to. At which of the following temperatures will a gas diffuse through a room most rapidly? Which of the following gases would have the fastest rate of diffusion, assuming all of the gases are at the same temperature? If the volume available to the gas is increased, the pressure exerted by one mole of gas molecules will. Which of the following is not a basic assumption of the Kinetic Theory? Gases consist of molecules in constant motion in straight-line paths. The temperature of gas is proportional to the average kinetic energy of the molecules.

The collisions between gas molecules and with the walls of the container are perfectly elastic. Since the collisions of molecules are perfectly elastic there is a strong attractive force between molecules in the gaseous state. All gases. John Charles. Robert Boyle. Which of the following expresses an inverse proportionality?

As P decreases, V increases. As n increases, P increases. Which of the following chemical systems has molecules that vibrate around in a fixed point in relation to the neighboring particles?

The gas law that describes the relationship between volume and number of moles is. Which of the following properties does not describe a gas? Which of the following indicates the amount of gas particles?

The partial pressure of an individual gas depends on the. Gas pressure is caused by:. If the volume of a confined gas is doubled while the temperature remains constant, what change would be observed in the pressure?

It would be half as large. It would double. It would be four times as large.The ideal gas law has some conditions that must be met, conditions that certainly cannot be met in the real world. These conditions include that the gases cannot interact with one another, gases must be moving in a random straight-line fashion, gas molecules must not take up any space, and gases must be in perfect elastic collisions with the walls of the container. These conditions minimize the effect that gas molecules have on one other, allowing a prediction based on completely random and unimpeded molecular movement.

In reality, these conditions are impossible. All real gas molecules have a molecular volume and some degree of intermolecular attraction forces. The container is expanded toand the temperature is increased to. In this case, two variables are changed between the initial and final containers: volume and temperature. Since we are looking for the final pressure on the container, we can use the combined gas law in order to solve for the final pressure:.

When using the ideal gas law, remember that temperature must be in Kelvin, not Celsius, so we will need to convert. At STP, an unknown gas has a density of. Based on this information and the periodic table, what is the identity of the gas in the container? Once again, we can use the ideal gas law in order to solve for the unknown gas. We will start again with the ideal gas law:. Density has the units of mass over volume, which means that we can rearrange the ideal gas law so that density is on one side of the equation.

However, we need to substitute one of the values so mass is also in the equation. Remember that moles are equal to mass divided by molar mass, so we can rewrite "n" in order to solve for density:.

STP means that the container is at 1 atmosphere of pressure and Kelvin. Knowing this, we can solve for molar mass:. Fluorine gas has a molar mass of As a result, we determine that fluorine gas is the unknown gas in the container. The container has a pressure of at a temperature of.

Based on this information and the periodic table, which of the following gases is in the container? In order to determine the gas being contained, we are going to need to rewrite the ideal gas law. The ideal gas law is written as follows:. The number of moles of a gas can be rewritten as the mass of the gas divided by its molar mass. Knowing this, we can rewrite the equation, and solve for the molar mass of the gas.

Use the given values in this equation to solve for the molar mass. Remember to first convert degree Celsius to Kelvin! Now that we have solved for the molar mass, we can see which gas has this molar mass on the periodic table. Argon has a molar mass of The combined gas law takes Boyle's, Charles's, and Gay-Lussac's law and combines it into one law.

It is able to relate temperature, pressure, and volume of one system when the parameters for any of the three change. Boyle's law relates pressure and volume:. Charles's law relates temperature and volume:.

Gay-Lussac's law relates temperature and pressure:. The ideal gas law relates temperature, pressure, volume, and moles in coordination with the ideal gas constant:. A scuba diver uses compressed air to breath under water.A gas is a state of matter with no defined shape or volume. Gases have their own unique behavior depending on a variety of variables, such as temperature, pressure, and volume.

While each gas is different, all gases act in a similar matter. This study guide highlights the concepts and laws dealing with the chemistry of gases. A gas is a state of matter. The particles that make up a gas can range from individual atoms to complex molecules. Some other general information involving gases:. Pressure is a measure of the amount of force per unit area. Gases with high pressure exert more force than gas with low pressure. The SI unit of pressure is the pascal Symbol Pa.

The pascal is equal to the force of 1 newton per square meter. This unit is not very useful when dealing with gases in real world conditions, but it is a standard that can be measured and reproduced. Many other pressure units have developed over time, mostly dealing with the gas we're most familiar with: air. The problem with air, the pressure isn't constant.

Air pressure depends on the altitude above sea-level and many other factors. Many units for pressure were originally based on an average air pressure at sea-level, but have become standardized. Temperature is a property of matter related to the amount of energy of the component particles.

Several temperature scales have been developed to measure this amount of energy, but the SI standard scale is the Kelvin temperature scale. The Kelvin scale is an absolute temperature scale and used in nearly all gas calculations. It is important when working with gas problems to convert the temperature readings to Kelvin. STP means standard temperature and pressure.

STP is commonly used in calculations involved with the density of gases or in other cases involving standard state conditions. At STP, a mole of an ideal gas will occupy a volume of Dalton's law states the total pressure of a mixture of gases is equal to the sum of all the individual pressures of the component gases alone.

The individual pressure of the component gas is known as the partial pressure of the gas. Avogadro's law states the volume of a gas is directly proportional to the number of moles of gas when pressure and temperature remain constant. Basically: Gas has volume. Add more gas, gas takes up more volume if pressure and temperature do not change. Boyle's gas law states the volume of a gas is inversely proportional to the pressure when the temperature is held constant. Charles' gas law states the volume of a gas is proportional to its absolute temperature when pressure is held constant. As the gas cools, the volume will decrease. Guy -Lussac's gas law states the pressure of a gas is proportional to its absolute temperature when the volume is held constant. As the gas cools, the pressure will decrease. The ideal gas law, also known as the combined gas lawis a combination of all the variables in the previous gas laws. Unfavorable conditions include high pressures and very low temperatures. Kinetic Theory of Gases is a model to explain the properties of an ideal gas. The model makes four basic assumptions:. Graham's law atates the rate of diffusion or effusion for a gas is inversely proportional to the square root of the molar mass of the gas.

The ideal gas law is a good approximation for the behavior of real gases. The ideal gas law fails when the pressure of the gas is very high or the temperature is very low.The ideal gas law is an important concept in chemistry. It can be used to predict the behavior of real gases in situations other than low temperatures or high pressures.

This collection of ten chemistry test questions deals with the concepts introduced with the ideal gas laws. If an additional 8 moles of the gas is added at constant pressure and temperature, what will be the final volume of the balloon?

A mixture of helium and neon gases is held in a container at 1. If the mixture contains twice as many helium atoms as neon atoms, what is the partial pressure of helium? If the vessel is allowed to expand isothermally to What is the final volume? The temperature of a sample of an ideal gas in a sealed 5. If the initial pressure of the gas was 3.

What is the pressure of the gas? How much faster or slower would oxygen effuse from a small opening than helium? What is the average velocity of nitrogen gas molecules at STP? When the leak was discovered, the pressure was reduced to 50 atm. How many moles of chlorine gas escaped? Share Flipboard Email. By Todd Helmenstine. Updated January 29, A balloon contains 4 moles of an ideal gas with a volume of 5.The state of matter in which inter-particle attraction is weak and inter-particle space is so large that the particles become completely free to move randomly in the entire available space, is known as gas.

In a laboratory, when hydrogen sulphide gas is prepared, it can be smelt even at 50 meters away. This is due to the phenomenon called Diffusion.

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The inter-particle or inter molecular spaces in a gas are very large. When hydrogen sulphide gas is produced, its particle collides with air particles. Due to the collisions of particles, they start moving in all possible directions. As a result of which the two gases mix with each other forming a homogeneous mixture of a gas. Thus, the released gas can be smelt to a long distance. Fit the wrapped nozzle tightly into a hole, bored half way through a rubber stopper.

Gradually, put more weight. The piston moves further downward and the volume of the air is further reduced. Now remove the weights one by one. You will notice that, on decreasing the pressure, the piston moves upward as such the volume of the air increases.

The molecular motion is directly proportional to the temperature. As temperature increases, molecular motion increases because the molecule possesses certain kinetic energy. And as the temperature decreases, molecular motion also decreases. Thus, when temperature is zero, molecular motion stops or ceases. Or Temperature remaining constant, the product of the volume and pressure of the given mass of a dry gas is constant.

According to Boyles law, on increasing pressure, volume decreases. The gas becomes denser. Thus, at constant temperature, the density of a gas is directly proportional to the pressure. At higher altitude, atmospheric pressure is low so air is less dense. As a result, lesser oxygen is available for breathing. This is the reason that the mountaineers have to carry oxygen cylinders with them. According to kinetic theory of matter, the number of particles present in a given mass and the average kinetic energy is constant.

If the volume of given mass of a gas is reduced to half of its original volume. The same number of particles will have half space to move. Alternatively, if the volume of a given mass of a gas is doubled at constant temperature, same number of molecules will have double space to move. Thus, number of molecule striking the unit area of the walls of container at a given time will become one half of original value.

This is the reason that:. According to kinetic theory of matter, the average kinetic energy of the gas molecules is directly proportional to the absolute temperature. Thus, when the temperature of a gas is increased, the molecules would move faster and the molecules will strike the unit area of the walls of the container more frequently and vigorously. If the pressure is kept constant, the volume increases proportionately.

Absolute or Kelvin scale of temperature. The value on the Celsius scale can be converted into Kelvin scale by adding to it. This act has led to the formulation of another scale known as Kelvin scale. The real advantage of the Kelvin scale is that it makes the application and the use of gas laws simple.WS Metric Conversions.

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## Ideal Gas Law Test Questions

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