Question

say wrong or correct number of molecules per unit volume increases with decrease in volume consequently number of collisions on the walls increases ​

Answer 1

Answer:

correct, When the volume of a gas is decreased at constant temperature the pressure increases.

Explanation:

The volume occupied by the molecules of the gas is negligible compared to the volume of the gas itself.

The molecules of an ideal gas exert no attractive forces on each other, or on the walls of the container.

Answer 2

Collision of gas molecules

Explanation:

• Adding air increases the number of gas particles in the tire. Collisions of particles with the inner walls of the tire create pressure from the enclosed gas.
• For this reason, the increasing number of air particles increases the number of collisions, which in turn increases the pressure in the tire.
• If the volume is reduced, the equilibrium will shift in favor of the direction in which fewer moles of gas are produced.
• As the volume increases, the equilibrium shifts in favor of the direction that produces more moles of gas. If the amount of gas in the container increases, the volume increases.
• If the amount of gas in the container decreases, the volume decreases. If you heat a gas, you give the molecules more energy so they can move faster. This means more effects on the container walls and more pressure.

Thus, collisions increase with increase or decrease in gas molecule volumes.