Why does diffusion occur, even when the pressure at both regions are equal
In: 4
Let’s start with a few details.
1- there is some of empty space between liquid and gas atoms. This allows them to move past each other.
2- materials with a temperature have vibrating or moving atoms. Hotter means more of then are moving faster.
3 pressure arises when there is a collision between two atoms. And this doesn’t cause then to stop moving, just bounce off and continue on a new direction.
So a group of atoms free to move (liquid it gas) had them in constant motion bouncing off each of their. They mill around, go past each other and such.
If they are all concentrated in one spot, but surrounded by a vacuum (no other atoms) this random motion means the atoms at the edge will face less obstacle in their outward direction, and will spread out.
If they are surrounded by a heavier gas there is resistance to this outward expansion. Even if there is pressure, and equal on both sides, that means the two sets are colliding. Our lighter gas is also smaller, and will bounce off the heavier gas… Into the Harris between them. The light gas will slip between the heavy atoms like cats in a crowd of people.
If surrounded by a lighter gas, the same commission that creates the pressure we measure well simply push the lighter atom away. The heavy atoms will just Wade through the light atoms, like people on a crowd of cats.
And it will spread out, on average, as collisions with the other gas impede the motion less than with the same gas. At least as long as the gasses have differing concentrations.
Edit: autocorrect weirdness
Latest Answers