The ideal gas equation states that: PV = nR T Given a situation in which the number of motes of gas that is being analyzed is held constant (as in today s lab where for both experiments trapped samples of gas are being analyzed) the equation can be written as: P_i V_i/T_i = P_fV_F/T_f where i and f represent initial and final conditions respectively. For Boyle's Law, what additional assumption is being made, and how Is the equation above modified? Do you think that this assumption for Boyle's Law is valid for today's experiment? Given Boyle's Law: a) Suppose two identical balloons are filled with 0.1 mole of helium, and one is taken to Miami and one to Denver. Which balloon would be bigger? (assume 85 degree F in both cities b) What would happen to the pressure of a gas sample if volume were increased to infinity (i.e. if the gas sample were released into space)?