1. The problem statement, all variables and given/known data A cylinder of compressed Oxygen is carried on a spacecraft headed for Mars. The compressed gas cylinder has a volume of 17000 L and is filled to a pressure of 248 atm at 231 K. The maximum pressure the cylinder can hold is 1000 atm.The contents of the cylinder are then entirely transferred to a partially filled holding tank of volume 10,000 L, originally at pressure 22 atm and 300 K. What is the new pressure in the holding tank at 300 K? 2. Relevant equations PV = nRT 3. The attempt at a solution Since we are given the initial pressure, I think we can can calculate the number of moles of gas in the tank before the transfer using PV = n RT. I did: (248 atm)(17,000 L) = n (0.0821) (231 K) n = 222,303.0725 moles Then I used this number and plugged it into the ideal gas law equation once more to come up with the new pressure. (P) (10,000 L) = (222,303.0725 moles)(0.0821) (300 K) P = 547.5324675 atm It says this is wrong, and I'm not sure why.