Increase in temperature of a gas filled in a container would lead to:

According to the Kinetic Theory of Gases, the average kinetic energy ($K.E.$) of gas molecules is directly proportional to the absolute temperature ($T$):
$$K.E.=\frac{3}{2}kT$$
Therefore, increasing the temperature leads to an increase in the kinetic energy of the molecules. Mass and intermolecular distance (for a constant volume container) do not change significantly with temperature alone. Pressure would actually increase, not decrease.