Question

1. Explain in terms of particle collisions and Dalton’s law why it can be assumed that the total pressure inside the gas collection tube is equal to the atmospheric pressure outside of the tube.

Answer 1

The gaseous particles that are inside the container exert a force on the walls of the container, on the other hand, the gaseous particles that are outside the container exert force. If there was less pressure from the inside, the tube would collapse.

Step-by-step explanation:

Dalton's law of partial pressures says that the total pressure in a mixture of gases is the sum of the partial pressures of its components. The partial pressure of each gas in a container is the pressure that the gas would perform if it were the only gas in that container. This can be assumed to be that there are no attractive forces between the gases inside the container.

Answer 2

The particles inside the container are exerting force on the walls of the container, while the particles outside of the container are also exerting force. If there were any less pressure from the inside, the tube would collapse. If there were any less pressure from the outside, the tube would explode. Hope it helps in any way.