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

Under what conditions will a gas be most likely to exhibit the ideal gas properties predicted by the ideal gas law? 1)high pressures and high temperature, because particles are forced closer together with higher kinetic energy, so intermolecular forces of attraction are weaker 2)high pressure and low temperature, because particles are forced closer together and moving slower, so the volume of the particles is less significant 3) low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker 4)low pressure and low temperature, because particles are spread farther apart with lower kinetic energy, so the volume of the particles is less significant