A gas occupies 22.4 l at stp and 14.5 l at 100c and 2.00 atm pressure. how many moles of gas did the system gain or lose?

At standard temperature and pressure 22.4 l of an ideal gas would contain 1 mole. in order to find the change in moles we must look at the ideal gas law PV=nRT where P=Pressure V=volume n=Moles R = Gas constant T = Temperature. To simplify this equation we will be using the gas constant at. 08206 L-atm/mol-K. We must first convert 100c to k which is 373.15. Then we can plug the values into our equation which gives us (2atm) (14.5 l) = (n) (.08206 L-atm/mol-K) (373.15). After some basic algebra we get the moles to equal roughly. 95 which is. 05 moles less than our original system.