AP Chemistry : AP Chemistry

Study concepts, example questions & explanations for AP Chemistry

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Example Questions

Example Question #321 : Ap Chemistry

A mixture of neon gas and argon gas is present in a container (container A). There are equal amounts of both gases in the container. A small pinhole is created in the container, allowing the gases to effuse into an empty container (container B). The effusion time is very brief, and the pinhole is eventually plugged, resulting in a mixture of both gases in both containers.

Suppose that after the pinhole is plugged, there are 100 argon atoms in container B. Approximately how many neon atoms would you predict to be in container B?

Possible Answers:

Correct answer:

Explanation:

We can compare the effusion rates of these gases using the following equation.

 

By calling neon "gas 1" and argon "gas 2," we can compare the effusion rates of the two gases by plugging their molecular masses into the equation.

This proportion is equal to the rate of neon effusion over the rate of argon effusion, giving the ratio of neon atoms to argon atoms in container B.

As a result, 141 atoms of neon gas will effuse out of the pinhole for every 100 argon gas atoms. Keep in mind that the heavier gas will effuse at a slower rate than the lighter gas; thus, we would expect there to be more neon than argon in container B.

Example Question #321 : Ap Chemistry

A 20cm tube holds two cotton balls, one in each end. The left cotton ball is saturated with undiluted HCl. The right cotton ball is soaked in an undiluted mystery compound. Vapors from the two cotton balls are allowed to mix within the tube.

Let us assume that the two compounds form a precipitate in the tube 6cm to the left of the right cotton ball. What is the molar mass of the mystery compound?

Possible Answers:

Correct answer:

Explanation:

This question is notably difficult, as it may not be immediately apparent what concept is being tested. As the vapors of the compounds mix and react, we are able to establish the distance the each vapor has traveled from the cotton ball into the tube in the given amount of time. The tube is 20cm, and the reaction takes place 6cm from the mystery compound cotton ball. From this, we can establish that in an equal amount of time the HCl vapor traveled 14cm and the mystery compound traveled 6cm.

In order to solve this problem, we use Graham's law to compare molar masses to the rates of diffusion of the two gases.

Since HCl moved 14cm to the right before interacting with the mystery compound, we know that the mystery compound moved only 6cm to the left. As a result, the diffusion ratio is 2.33.

Now, we need to find the square root of the inversed molar masses, which equals this diffusion ratio.

So, the molar mass of the mystery compound is 198 grams per mole. This makes sense, because larger gases will move more slowly compared to lighter gases. 

Example Question #2 : Effusion

Which of the following gases has the highest rate of effusion?

Possible Answers:

Correct answer:

Explanation:

The rate of effusion of a gas is inversely proportional to the square root of the molecular weight of the gas.

The lighter a gas is, the faster it will effuse; the heavier a gas is, the slower it will effuse.

Of all the choices, helium (He) has the lowest molecular weight (atomic weight in this case), so it will have the highest rate of effusion.

Example Question #1 : Effusion

Gas A has a molar mass that is  times greater than that of Gas B. Which of these gases would be expected to effuse through a small hole faster? By how much?

Possible Answers:

Gas B effuses  times faster than Gas A

Gas A effuses  times faster than Gas B

Gas B effuses  times faster than Gas A

Gas A effuses  times faster than Gas B

Correct answer:

Gas B effuses  times faster than Gas A

Explanation:

In order to answer this question, let's start by considering what effusion is and what things affect it. Effusion is the movement of a gas through a tiny hole that separates two different spaces. Because the gas particles move around in random directions with an average speed that is dependent on the temperature of the sample, lighter gas particle will move faster than heavier gas particles. This is because at a given temperature, all gas particles in a sample will have the same average kinetic energy. Consequently, we would expect gas particles with a higher molar mass to effuse more slowly than gases with a lower molar mass. This means that Gas B should effuse faster than Gas A.

The next step is to actually calculate how much greater Gas B effuses compared to Gas A. To do this, we'll need to use the following equation:

Since we know that Gas A is  times heavier than Gas B, we can plug this into the equation to solve for the ratio of Gas B's rate of effusion to that of Gas A.

Therefore, Gas B effuses  times faster than Gas A.

Example Question #1 : Gases

How much faster/slower the rate of effusion for oxygen gas compared to hydrogen gas?

Possible Answers:

2 times faster

2 times slower

4 times slower

4 times faster

16 times slower

Correct answer:

4 times slower

Explanation:

Rate of effusion:

 and  must be used because they exist as bimolecular molecules. The correct answer is that Oxygen gas will effuse 4 times slower than hydrogen gas.

Example Question #2 : Gases

COCl2 (g) ⇌ CO (g) + Cl2 (g)

Initially a reaction chamber contains only 2 moles of COCl2, after the reaction has reached the equilibrium shown above the pressure is measures to be 2.60 atm.  What is the most likely cause for the increase in pressure?

Possible Answers:

Heat is consumed during the course of the reaction

CO is larger than COCl2

CL2 is a diatomic gas

There are more molecules in the chamber, increasing the liklihood of atomic collisions with the wall of the container leading to increased pressure.  

Heat is released during the course of the reaction

Correct answer:

There are more molecules in the chamber, increasing the liklihood of atomic collisions with the wall of the container leading to increased pressure.  

Explanation:

The equilibrium expression indicates that one mole of COCl2(g) will decompose into CO (g) and Cl2 (g).  One mole of gas is present on the left side of the equation, and two moles of gas are present on the right side of the equation.  The increases in pressure is due to the increase in the number of gas molecules in the reaction chamber.  

Example Question #1 : Other Gas Concepts

A gas is at STP

What does STP refer to?

Possible Answers:

0 C, 1 atm

0 C, 25 atm

25 C, 25 atm

25 C, 1 atm

298 K, 25 atm

Correct answer:

0 C, 1 atm

Explanation:

Standard temperature and pressure is 00C and 1 atm

Example Question #2 : Other Gas Concepts

What is the molar mass of a gas with a density of at STP?

Possible Answers:

Correct answer:

Explanation:

Since we have the density of the mystery gas, we can rearrange the ideal gas law so that the remaining factors are equal to the density of the gas.

We can redefine moles of gas as mass over molar mass.

We can now rearrange the equation to solve for density (mass per volume), which is given in the question.

Using this set up and the values for standard temperature and pressure, we can solve for the molar mass.

Example Question #13 : Gases

Which of the following will not be found in the atmosphere for an extended period of time?

Possible Answers:

Correct answer:

Explanation:

Most gases exist as diatomic molecules in nature. , and  are all common gases found in the atmosphere and the air we breathe.

Ozone, , is a rare exception to the diatomic bonding principle, and is also found in significant quantities in the atmosphere.

Monatomic oxygen, , has only six valence electrons and is relatively unstable; this compound would not be found naturally in the atmosphere.

Example Question #11 : Gases

A flexible box contains four moles of octane gas at STP with an excess of oxygen. If the octane is combusted according to the following reaction and the box is allowed to expand, what is the change in volume?

Possible Answers:

The size of the box increases by 

More information is needed in order to solve

The size of the box increases by 

The size of the box increases by 

Correct answer:

The size of the box increases by 

Explanation:

This question does not acually deal with the ideal gas law, but only with the standard volume of a gas at STP. At standard temperature and pressure, one mole of gas has a volume of 22.5L.

We know that initially we have four moles of octane and excess oxygen. This means that octane will be the limiting reagent for the combustion reaction, since oxygen is in excess.

The total moles of reactant gas when utilizing all four moles of octane is 54, while the total moles of product gas is 68.

There is a total change in moles of:

Since we end the reaction with 14 more moles of gas than we started, the volume must increase:

The change in volume is .

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