1. The problem statement, all variables and given/known data What is the density of nitrogen gas (molecular mass = 28 u) at a pressure of 1.7 atmospheres and a temperature of 332 K? 2. Relevant equations You must convert pressure from atmospheres to Pascals. I'vedone this using the conversion 1 atmosphere = 1.01*10^5 pascals. I was also told that I needed to convert molecular mass into kilograms. Given a molecular mass of 28u. I calculated the mass in kilograms to be 0.00002799 kg/mole of Nitrogen. 3. The attempt at a solution 1 molecule of Nitrogen = 28u 28u * 1.066*10^-27=4.648*10^-26 grams per molecule. 1 mole = 6.022*10^23 molecules therefore 1 mole = 0.027990256 grams. There are 1000 grams in 1 kg. So 1 mole = 0.00002799 kg of Nitrogen. volume=nRt/p If I assume 1 mole and am given R=8.31 t=332k and p=1.7 atmospheres My equation should come to be volume = (1)(8.31)(332)/171700. This gave me a volume of approximately 0.01607 If I then divide my mass in kilograms by this I get 0.00175 as my density which is wrong. Am I missing a step? Am I using the wrong equations? Thanks in advance for any help you can offer!