30-04-2021

Example Of Avogadro's Law In Real Life

Avogadro's Law Problems And Answers
Example Of Avogadro's Law In Real Life Pdf
Example Of Avogadro's Law In Real Life

How is Avogadro's law used in everyday life?

For example, air is a mixture of gases which contain about 80% nitrogen and 20% oxygen; although small amounts of other gases are present as well. According to Dalton's law, the partial pressure exerted by the nitrogen oxygen which make up the air will be equal to the total pressure of the air; and will increase simultaneously. This blog is created as part of Faith Committee’s Performance Task in Science 10. It is all about Amedeo Avogadro’s Gas Law; what it is, and some real life examples of it. We aim to explain the assigned gas law to the readers. To navigate, please use the sidebar found on the upper right corner of Read more 'Welcome!' Avogadro’s law (now known as Avogadro’s hypothesis) was first published in 1811 and is one of the main theories that helped to build the foundation for the ideal gas laws. These laws help to explain the relationship that gases have between the number of molecules and the volume of the container they fill. Gases laws with examples kinds of gas laws gay-lussacs law avogadros law finding the temperature in gas laws charles law practical situation in amontons law 5 example of daltons law examples of amontons law volume and temperature examples Examples on Amontons Law of Gases amontons law examples practical application of daltons law.

1 Answer

Avogadro's Law states that the volume of a gas is directly proportional to the number of moles of gas.

Here are some examples.

As you blow up a basketball, you are forcing more gas molecules into it. The more molecules, the greater the volume. The basketball inflates.

A flat tire takes up less space than an inflated tire, because it contains less air.

Lungs expand as they fill with air. Exhaling decreases the volume of the lungs.

A balloon filled with helium weighs much less than an identical balloon filled with air. Both balloons contain the same number of molecules. Helium atoms have lower mass than either oxygen molecules or nitrogen molecules in air, so the helium balloon is lighter.

Hope this helps.

Avogadro’s Law

Avogadro’s law states that –

“At the similar and constant physical conditions like Temperature and Pressure, the two different gases like hydrogen and nitrogen in the same volume contain an equal number of molecules.”

How was Avogadro’s Law Influential?

Avogadro’s law was able to explain how equal volumes of gases at ideal conditions gave an equal number of molecules. Although scientists at that time rejected this hypothesis, it gained acceptance after his death, when other scientists realized how important and revolutionary it was in the field of science. You can understand this law with Avogadro’s Law Examples, Lungs, Tyres, etc.

Mathematical Derivation of Avogadro’s Law

From the Ideal Gas Equation,

PV=nRT

Avogadro's Law Problems And Answers

Where, P = Pressure, T = Temperature, n = number of molecules of the gas, V = volume of the gas, R= Ideal gas constant (also known as Boltzmann Constant = 0.082057 L atm K-1 mol-1)

Assume P & T = Constant

V = n (RT/P)

Where, K = RT/P (Proportionality constant)

V α n

The above equation says that as the volume is increasing, the number of molecules of the gas is also increasing. Or As the volume decreases the number of molecules of the gas is also decreases (like in Ballons). Although Avogadro’s Law can be written in a lot of ways, this relation is the easiest to understand.

At condition 1 (at constant temperature and pressure),

At Condition 1, the Volume of gas is denoted as V₁and the number of molecules of a gas is denoted as n₁.

At Condition 2 (P, T = Constant)

At Condition 2, the Volume of gas is denoted as V_2,and the number of molecules of a gas is denoted as n₂.

According to Avogadro’s law,

V₁/n₁ = V₂/ n₂ ————————————————————-(a)

Assume volume V2 is the twice of the volume V1, So,

V₂= 2V₁ ———————————————————————(b)

Put Value of V2 in equation number (a)

V₁/n₁ = 2V₁ / n₂

n₂ = 2n₁ ——————————————————————–(c)

According to equation (c ), If the number of volumes is doubled, then the number of molecules of a gas is also doubled.

Note: This law is for Ideal gases. In real gases, slight variations and deviations occur.

What is Avogadro’s number?

The Scientist Avogadro did not discover Avogadro’s number. The number of molecules in 1 mole is known as Avogadro’s number. Its value in the SI unit is 6.02214129 ×1023 mol-1. And it is denoted by N_A. Nowadays, Avogadro’s constants are used instead of Avogadro’s number.

Avogadro’s Graph

Graphical representation of Avogadro’s law,

The above graph is plotted (shows linear relationship) between volume and mole at the constant physical condition. As the volume is increasing, then the molecules are also increasing.

Real-World Avogadro’s Law Examples

Since Avogadro’s law is for ideal gases, people think that it does not have any real-world Avogadro’s Law Examples and that it is just a hypothesis. But that is not the case. Avogadro’s law has numerous real-world applications, and it explains a lot of things that go on in our day to day life.

Lungs

The first real-world Avogadro’s law examples can be seen in our own body. We all know that the lungs help us in breathing. But have we ever wondered about the mechanism? Thanks to Avogadro’s law, it’s easier to understand how our Lungs work.

When we breathe in (inhale), air flows inside our lungs, causing the lungs to expand (increase in volume). From our lungs, the oxygen is extracted and injected into our bloodstream. Then, we breathe out (exhale), causing the Carbon Dioxide (CO2) to pass through, and thus shrinking the volume of the lungs.

Sports

All of us love to play games, right? No? Are you not into sports? It doesn’t matter, but if you’re looking for Avogadro’s law examples, you will find them in games like Football and Basketball. When you blow air into a ball, it causes the volume of the ball to increase, as air molecules start to collect inside of it. And if you puncture the ball, all that air will come out with pressure, causing the ball to shrink and create a loud sound. Avogadro’s law comes into play to explain to us all the things that are going on here.

Tires

Everyone found yourself in a situation where you got stuck in the middle of the road because of a flat tire? Well lucky if you haven’t. Things like puncture, temperature, or time can cause the tire to lose the air inside it, which decreases the volume of the tire and ruins your trip. When you take your car to the gas station, you also get the tires checked. When air is blown into the tires, they get inflated, and the volume is increased, and your car can move smoothly. This is another of Avogadro’s Law Examples.

Balloons

One more Avogadro’s Law Examples is a balloon. Everyone loves balloons. And to bring them to that beautiful state, you have to force air from your mouth into the balloon, causing it to expand to a much higher volume.

Limitations of Avogadro’s Law

Although Avogadro’s law has numerous real-world applications (Avogadro’s Law Examples discussed above) if it also has a lot of limitations. This doesn’t mean that Avogadro’s Law is not accurate; it just means that it is not perfect. So some of the limitations of Avogadro’s Law are listed below,

The biggest limitation of Avogadro’s Law is that it was introduced to the world, taking into account that it works best for ideal gases. But such a thing as an ideal gas doesn’t exist in the real world. To get perfect and accurate answers, you have to apply this law to ideal gases. For real gases, this law still answers, but the accuracy is often questionable.
Calculation of Heavy molecules tends to give poor and inaccurate results as compared to lighter gas molecules. This is where the limitation of Avogadro’s law is observed since the calculations for some major heavy molecules turn out to be slightly, or sometimes, mostly inaccurate.
In real gases, temperature plays a significant role in increasing the ratio of volume to the mole as compared to ideal gases. This is because, in real gases, a temperature increase causes the gas to expand because of the intermolecular repulsion forces.