Question

Chapter 5: Complete for a thumbs up!

1. Explain the difference between an ideal gas and a non-ideal gas. Use examples.

2. You mix 760 mmHg of pure nitrogen gas into a container of pure oxygen gas. The total pressure is 1010 mmHg after the addition is complete. What is the partial pressure of oxygen?

3. Manipulate the ideal gas law to find equations solely for; pressure, volume, temperature, and moles.

4. Explain all of the consequences that occur after increasing the volume of a cylinder full of oxygen gas from 50 mL to 500 mL. What happens to all other aspects of the ideal gas law? No need to calculate, just predict what will happen

Answer 1

Q1. Real gases-

- have small attractive and repulsive forces between particles.

- have a volume of gas particles.

- real gas particles collide in -elastically.

- Example - N2 , O2 , CO2 , CO, He etc.

Ideal gases-

- No force between particles of ideal gases.

- have no volume.

- Ideal gas particles collide elastically.

- Ideal gas do not exist, it is only theoretical model.

A real gas behaves like ideal gas at high temperature and low pressure.

A real gases deviate from ideal behavior at high pressure and low pressure.

-Ideal gas equation - PV =nRT

-real gas follows the equation- (P + a / V2 ) (V- b) = nRT

Q4. Acc. to Boyle's law - V $\alpha$ 1/ P

If we increase volume then pressure of the gas will decrease.

As according to question volume increase from 50 ml to 500 ml, then pressure will decrease respectively.

b) Total press N₂ - 760 mm ny + Pure og gop find out partial prin of op Daltons law of partial press To lo lolo mom ng = 760 mm of Mg + 1 Po = 10lo-760 - 250 mm of rg

Derivation of the Acc. to Boyle's law Ideal gor Equation- Ace to Acc. to Charles low- TO Avogadras law- - van ing from above equations - * له لا prant pvz MRT R = universal gop = 8.3145/mol-k constant