Question

Which of the following statements is true for ideal gases, but is not always true for real gases?

Answer 1

Answer:

C. Replacing one gas by another under the same conditions, has no effect on pressure.

Explanation:

Ideal gas:

 A gas is treated as an ideal gas if temperature is high and pressure is low.

Kinetic energy for ideal gas given as

$K.E.=\dfrac{3}{2}KT$

So when temperature of gas is increases then  Average molecular kinetic energy will also increases.

The size of molecule is negligible as compare to the dimension of container. It mean that volume occupied by molecule is less as compare to the volume of container.

The between molecules is perfectly elastic.

Ideal gas equation

P V = m R T

So the option C is not always true.