We start in situation A with 1 mole of an ideal gas in the right bulb with the valve closed. The gas has a pressure, volume, and temperature we symbolize by pA, VA, TA. Then the gas spreads out to occupy both sides. Once it has settled down we have situation B with parameters pB, VB, TB. Since there is nothing opposing the motion of the gas into the larger volume, this is called a free expansion. How does the volume and temperature compare in systems A and B. Place the appropriate coefficient in the blank

Free expansion is also known as the joule expansion, this happens when a gas does not have an expansion limit and its volume increases until it is allowed.

That is why as the initial volume passes at the end the pressure decreases since the molecules are more distant from each other without a barrier that stops or compresses them.

It is an irreversible process and the equation would be:

Initial pressure X Initial volume = Final pressure X Final volume

Explanation:

Where P is the pressure, V is the volume, and i and f refers to the initial and final states. Since the gas expands, Vf> Vi, which implies that the pressure drops (Pf <Pi).

i wish i could but this one is weird give me abc and i can solve it.