Here we're told that a 500 milliliter container at a pressure of 600 milliliters of mercury possesses 29.3g nitrogen gas at 50�C. Here we need to determine the correct units needed for the ideal gas law. So remember the ideal gas law is PV=nRT, so P stands for pressure. Remember, pressure needs to be in units of atmospheres. So here we're going to do a conversion. We're going to go from 600mm of mercury into atmospheres. Millimeters of mercury go here on the bottom and then atmosphere go here on top. Remember the relationship is that for everyone atmosphere it's 760mm of mercury. So when we do that we're going to get a pressure of 0.789 atmospheres.
Although 600 has one sick figs, let's just go with three sig figs here just so that we don't have just .8 as atmospheres. Next volume volume needs to be in liters, so we have 500 milliliters. And remember 11 milli equals 10 to the -3. So this would just come out as oh point 500 liters. Next we need moles. So moles is N Remember nitrogen gas, nitrogen. It's natural or a standard state is N2. It's one of our diatomic molecules, so we're told that we have 2029 .3G of N2. We got to convert that into moles SO1 mole of N2.
So there's two nitrogens. According to the periodic table, each one is 14.01g, so multiplying that by two gives me 28.2g for the combined weight in north 2. So grams here cancel out and I'll have my moles here. We'll put it as 1.05 moles of N2 and then finally we need our temperature, ours our constant, so we don't have to worry about giving the correct units. It's 08206 like we said earlier, so temperature here needs to be in Kelvin. So remember to go from Celsius to Kelvin you're supposed to add 273.15. Sometimes professors will just say plus 273, but if you want to be as accurate as possible you want to put 273.15. So when you add that, that's three 23.15 Kelvin.
So here we have all of the units that we need in the correct forms. So just remember ideal gas law and what are the correct units that we need to utilize for each one of these variables?