## What are the gas laws and their formulas?

The equations describing these laws are special cases of the ideal gas law, PV = nRT, where P is the pressure of the gas, V is its volume, n is the number of moles of the gas, T is its kelvin temperature, and R is the ideal (universal) gas constant.

### What are the 5 types of gas laws?

The five main gas laws in chemistry are Boyle’s Law, Charle’s Law, Gay Lussac’s Law, Avogadro’s Law and Ideal Gas Law.

**What are some real life examples of Boyle’s Law?**

You can observe a real-life application of Boyle’s Law when you fill your bike tires with air. When you pump air into a tire, the gas molecules inside the tire get compressed and packed closer together. This increases the pressure of the gas, and it starts to push against the walls of the tire.

**What is a real life example of Avogadro’s law?**

Avogadro’s Law in Everyday Life When you blow up a balloon, you are adding molecules of gas into it. The result is that the volume of the balloon increases – and in order to do this, you decrease the number of molecules in your lungs (which decreases their volume)! A bicycle pump does the same thing to a bicycle tire.

## What law is blowing up a balloon?

An example of Boyle’s law in action can be seen in a balloon. Air is blown into the balloon; the pressure of that air pushes on the rubber, making the balloon expand. If one end of the balloon is squeezed, making the volume smaller, the pressure inside increased, making the un-squeezed part of the balloon expand out.

### Is breathing an example of Avogadro’s law?

Breathing Human lungs demonstrate Avogadro’s law in the best possible way. When we inhale, the lungs expand because they get filled with air. Similarly, while exhaling, the lungs let the air out and shrink in size.

**How do you remember Henry’s Law?**

Henry’s Law: The solubility of a gas increases with pressure. To remember good old Hank, remember the bubbles in the shaken Coke you drank.

**What law is V1T1 V2T2?**

Charles’s law states that temperature and pressure are directly proportional. This means if temperature increases, then pressure will also increase. On the other hand, if temperature decreases, then pressure will also decrease. The equation for comparing two samples of a gas using this law is V1T1=V2T2.