Question

The diagrams show gases that are stored in two separate but similar containers.

2 identical containers have gas particles, represented by small balls with arrows representing movement in random directions. The Gas 1 container has many fewer balls than the Gas 2 container.
If both gases are at the same temperature, which one has the greater pressure?
gas 1 because the particles are moving much faster
gas 1 because it has fewer particles that are close together
gas 2 because it has more particles that are colliding
gas 2 because the particles have more space between them

Answer 1

Gas 2, because it has more particles that are colliding.

At the same temperature the particles have the same average speed (same kinetic energy), so pressure depends on how many collisions hit the walls. More particles (higher n or N) -> more collisions per unit time -> higher pressure (p = NkT/V).