i) Commercially, nitrogen is sold as compressed gas in cylinders. If a cylinder of volume 116 L is filled with N2 to a pressure of 1.38 x 104 kPa at 298.15K, what mass of N2 does the cylinder contain? Assume ideal gas behaviour. Answer: Mass N2 = 18104 g = 18.1 kg ii) Now, regarding part i), if the tap were opened and the gas allowed to escape, how many litres of N2 gas at 100 kPa and 298.15K would come out of the cylinder. Answer: Volume at 100 kPa = 16008 L. But, 116 L remains in the container, so Vol gas escaped = 16008 – 116 = 15892 L = 1.59 x 104 L For part ii), the answer was found by finding the total volume that could be contained in the environment using pV = nRT, and then subtracting 116 L from that total since that much is still remaining. Now, my question is: Is it possible to find the actual amounts (in moles) of N2 in the cylinder and outside, respectively? I am wondering this b/c the actual pressure in the environment would no longer be exactly 100 kPa since 116 L was removed in terms of nitrogen gas, and now the pressure is not exactly 100 kPa nor is the amount what we originally stated when using pV = nRT. With the pressures and amounts of nitrogen gas now unknown in the cylinder and environment due to the subtraction of 116 L, is there any way to actual find these variables? Was there an error in my logic? Thanks!