What is the difference between the Van Der Wals equation and the Ideal Gas Law?

Answer 1

First, the Ideal Gas Law is the equation for ideal gases. I assume you know that ideal gases have negligible forces of attraction and that they are independent of each other. (PV=nRT)

The Van Der Waals equation is the modified Ideal Gas Law
equation that can describe the properties of REAL gases. Real
gases only exhibit ideal gas properties when they are in low
pressures and high temperatures.

The two's are exponents. They are raised to the second power. (P - n2a/V2)(V-nb) = nRT

a, n, b are values for different gases.

Ideal Gas Law = ideal gases
Van der Waals = real gases

Answer 2

The assumptions of the ideals gas law are: 1) molecules are point masses 2) molecules occupy no volume 3) when molecules collide they conserve kicnetic energy(elastic collision) 4) there are no intermolecular attractions So the van der waal's equation reduces to the ideal gas law for small monoatomic gases at high pressure and low pressure

Answer 3

Van Der Wals equation takes into account forces between particles of gases

Answer 4

First it's van der Waals' equation.
It has two "fudge factors" these take into account forces between molecules and the fact that the molecules occupy some space within the gas.