If one were to fill a soccer ball with hotter than room temperature air they would have to refill ball because once the air molecules have cooled down they won't be as excited and will lose pressure.  This can be seen using the ideal gas law equation, PV = nRT .  In the soccer ball, the volume (V), number of molecules (n), and the universal gas constant(R) are all constant.  This allows us to set the initial pressure and temperature equal to the final pressure and temperature and get P_i/T_i=P_f/T_f .  Now we have the hot initial temperature which gives us an initial pressure, so when the air cools to the final temperature (T_f) we see that the pressure decreases, because T_f decreases, and thus will require someone to refill the soccer ball so that it will be inflated properly.