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Pressure and Density

Have you tried to pop a balloon? If you step or sit on one, it will eventually pop with a loud "bang", scaring anyone close enough.

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# Pressure and Density

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Nie wieder prokastinieren mit unseren Lernerinnerungen. Have you tried to pop a balloon? If you step or sit on one, it will eventually pop with a loud "bang", scaring anyone close enough.

But why does it pop? Balloons pop because of the relationship between pressure and density (or more specifically, pressure and volume). In this article, we will learn about the relationship between pressure and density, so keep reading to learn the answer to our query!

• First, we will define pressure and density
• Then, we will look at the relationship between pressure and density
• Next, we will look at the Ideal Gas Law and how it relates to pressure and density
• Lastly, we will work on some examples related to pressure and density

## Pressure Definition

Pressure is the force exerted by one substance onto another, divided by the area of the receiving substance. For a gas, pressure is the force exerted by a gas onto the walls of its container, divided by the area of the container.

An ideal gas is a hypothetical gas that approximates the behavior of "real gases". The properties of an ideal gas are:

• Negligible volume
• Negligible mass
• No interactions between particles
• Fully elastic collisions (no loss in kinetic energy)
• Particles are in constant motion

From now on, when we mention gases, we are referring to ideal gases.

So, how does the gas exert this pressure? The answer is collisions. Ideal gases are in constant motion and can move in every direction. Because of this, they are bound to collide with each other and the walls of their container. When a gas particle collides with the container, it exerts a force onto it, then bounces off. The greater the number of collisions, the greater the pressure.

Below is a diagram of this process: Fig.1-Gas particles collide with the container to create pressure

The gas particle particles with the lines coming off them are colliding with the container and are about to bounce back off. The other particles in the container are also moving and can also collide with the container at a later time

## Density Definition

Now, let's look at the definition of density.

Density is a substance's mass per volume (m/V). For gases, we often use the number density, which would be the number of moles (n) per volume (n/V).

Density answers the question, "How much of this substance is contained within this volume?"

Below is an example of what density looks like for gases: Fig.2-When the volume is the same, more moles=higher density

For gases, the formula for density is:

$$\frac{n}{V}$$

Where n is the number of moles and V is volume

Since the volume for each sample is the same, the container with more gas particles (right) has a greater density.

## Relationship Between Pressure and Density

Pressure and density have a direct relationship, meaning that if one increases, so does the other.

To put it mathematically:

$$P \propto \frac{n}{V}$$

Where P is pressure, n is the number of moles, V is volume, and ∝ is the symbol for "proportional to"

This also means that pressure is directly proportional to the number of moles, but inversely proportional (one goes up, the other goes down) to volume, since volume is in the denominator.

When volume increases, the total density decreases, which is why there is the inverse relationship between pressure and volume

So, why is this? Well, let's think back to our definitions. Pressure is based on two things: the number of collisions (i.e. more collisions equals greater force) and the area of the container.

If the volume is stable, and the number of moles increases (net increase in density), the number of collisions is also going to increase. Fig.3-An increase in density due to an increase in moles causes an increase in pressure

Basically, the particles have less room to move freely, which increases the likelihood of a collision.

Now let's talk about what happens when volume is changed (number of moles is stable). If the volume is decreases, not only will the area decrease, but the number of collisions will increase as well. Fig.4-When volume decreases (density increase), the pressure increases

Pressure is force/area, so a decrease in volume leads to an increase in pressure (more collisions due to less space) and a decrease in the area.

In our introduction, I talked about popping balloons. The reason why the balloon pops is because of this relationship. When you step/stand on the balloon, you are decreasing the volume, so the pressure must increase. When the pressure gets too much for the balloon to withstand, it bursts.

## Ideal Gas Law

The relationship between pressure and density is shown by the Ideal Gas Law.

The ideal gas law is used to show the behaviors of ideal gases, and therefore approximate the behavior of real gases.

The formula is:

$$PV=nRT$$

Where P is pressure, V is volume, n is the number of moles, R is the Gas Constant, and T is temperature

Let's rearrange this formula, so it clearly shows the relationship between pressure and density

$$PV=nRT$$

$$P=\frac{nRT}{V}$$

$$P=\frac{n}{V}*\frac{RT}{V}=Density\cdot \frac{RT}{V}$$

As you can see, the ideal gas law shows that pressure and density (n/V) are directly proportional.

## Pressure and Density Examples

Now that we understand the relationship between pressure and density, let's work on some examples!

A 0.56 L balloon contains 1.35 mol of helium. If the same amount of helium was pumped into a 0.76 L balloon, which balloon would have the greater pressure?

Let's look at our relationship:

$$P \propto \frac{n}{V}$$In this case, volume (V) is increasing. Since pressure and volume have an inverse relationship, the 0.56 L balloon would be the one with the greater pressure

At 1 atmosphere and 0 °C, helium has a density of 0.179 g/L. If the pressure is raised to two atmospheres, what will happen to the density?

Let's take another look at our formula:

$$P \propto \frac{n}{V}$$

Since pressure is directly proportional to density, an increase in pressure means there will also be an increase in density

Let's do one more, shall we?

A 2.5 L container (container A) of hydrogen has a pressure of 1.35 atm. Another container (container B) of hydrogen is 3.2 L, with a pressure of 1.14 atm. Which container has more moles of hydrogen?

Let's rearrange our equation, so we can see this relationship better:

$$P \propto \frac{n}{V}$$

$$PV \propto n$$

So the product of pressure and volume is directly proportional to moles, meaning that whichever box has the larger product will have more moles of gas

$$PV \propto n$$

$$(1.35\,atm)(2.5\,L) \propto n$$

$$3.375\,atm*L \propto n$$

$$PV \propto n$$

$$(1.14\,atm)(3.2\,L) \propto n$$

$$3.648\,atm*L \propto n$$

Since container B has a greater pressure-volume product, it will have more moles of hydrogen

## Pressure and Density - Key takeaways

• Pressure is the force exerted by one substance onto another, divided by the area of the receiving substance. For a gas, pressure is the force exerted by a gas onto the walls of its container, divided by the area of the container.
• Density is a substance's mass per volume (m/V). For gases, we often use the number density, which would be the number of moles (n) per volume (n/V).
• Pressure and density have a direct relationship, meaning that if one increases, so does the other.

To put it mathematically:

$$P \propto \frac{n}{V}$$

Where P is pressure, n is the number of moles, V is volume, and ∝ is the symbol for "proportional to"

• This also means that pressure is directly proportional to the number of moles, but inversely proportional (one goes up, the other goes down) to volume, since volume is in the denominator.

Pressure is due to gas particles colliding with the walls of their container. When density increases, the number of particles per volume increases, so the likelihood of collisions increases. This therefore causes an increase in pressure.

Using the ideal gas law, we can relate pressure to density. The ideal gas law is:

PV=nRT

Rearranging this we get,

P=(n/V)*(RT/V)

P is pressure and n/V is density, so this equation shows us that these variables have a direct relationship.

Pressure is the force exerted by one substance onto another, divided by the area of the receiving substance. For a gas, pressure is the force exerted by a gas onto the walls of its container, divided by the area of the container.

Density is a substance's mass per volume (m/V). For gases, we often use the number density, which would be the number of moles (n) per volume (n/V).

The formula for density is:

p=m/V

Where p is density, m is mass, V is volume

For gases, we often use the number density:

p=n/V

Where n is the number of moles

## Pressure and Density Quiz - Teste dein Wissen

Question

What is pressure?

Pressure is the force exerted by one substance onto another, divided by the area of the receiving substance. For a gas, pressure is the force exerted by a gas onto the walls of its container, divided by the area of the container.

Show question

Question

What is density?

Density is a substance's mass per volume (m/V). For gases, we often use the number density, which would be the number of moles (n) per volume (n/V).

Show question

Question

What is the formula for number density?

$$\frac{n}{V}$$

Show question

Question

Which of the following represents the relationship between pressure and density?

$$P \propto \frac{n}{V}$$

Show question

Question

True or False: Pressure and volume are inversely proportional

True

Show question

Question

True or False: Pressure and the number of moles are inversely proportional

False

Show question

Question

What factors affect pressure? (i.e. what variables are used to calculate pressure)

Number of collisions and the area of the container

Show question

Question

What is the formula for the ideal gas law?

$$PV=nRT$$

Show question

Question

What is an ideal gas?

An ideal gas is a hypothetical gas that approximates the behavior of "real gases"

Show question

Question

Which of the following is NOT a property of an ideal gas?

Interactions between particles

Show question

Question

Why does a balloon pop when stepped on?

The volume decreases, which causes an increase in pressure. The balloon pops when the pressure is too much for it to handle

Show question

Question

True or False: The relationship between density and pressure is based on the identity of a gas

False

Show question

Question

A 2.5 L container (container A) is filled with 2.1 moles of hydrogen. Another container (container B) is 1.7 L and contains the same amount of gas. Which container has the higher pressure?

Container B

Show question

Question

A 3.4 L container of neon gas (container A) has a pressure of 1.2 atm. Another container (container B) has a volume of 2.7 L and a pressure of 1.6 atm. Which container has more moles of neon gas?

Container A

Show question

Question

Gas A has a density of 0.21 mol/L and gas B has a density of 0.35 mol/L. Which gas has a greater pressure?

Gas B

Show question

## Test your knowledge with multiple choice flashcards

Which of the following represents the relationship between pressure and density?

True or False: Pressure and volume are inversely proportional

True or False: Pressure and the number of moles are inversely proportional

Flashcards in Pressure and Density15

Start learning

What is pressure?

Pressure is the force exerted by one substance onto another, divided by the area of the receiving substance. For a gas, pressure is the force exerted by a gas onto the walls of its container, divided by the area of the container.

What is density?

Density is a substance's mass per volume (m/V). For gases, we often use the number density, which would be the number of moles (n) per volume (n/V).

What is the formula for number density?

$$\frac{n}{V}$$

Which of the following represents the relationship between pressure and density?

$$P \propto \frac{n}{V}$$

True or False: Pressure and volume are inversely proportional

True

True or False: Pressure and the number of moles are inversely proportional

False

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