<p>How many moles of Nitrogen gas are there in 0.38 liters of gas at 0C and 380 mm Hg pressure ? </p>
<p>im having a hard time with this one so feedback would be appreciated!</p>
<p>Ideal gas law.</p>
<p>PV=nRT</p>
<p>You're given P, V, and T... and R is a constant. Solve for n. Don't forget to convert temperature to Kelvins and pressure to atm.</p>
<p>Solve using PV=nRT making sure you convert T to kelvins. Should be simple to solve after that.</p>
<p>EDIT: LOL goldshadow you beat me by 10 seconds.</p>
<p>okay i did that but i keep getting the wrong answer according to the book (barrons)</p>
<p>n= (.5atm)(.38L)/(.220)(273K) =0.0085 ( thats how the book wrote it i think the .220 should have been .0821 the R constant right ?? )</p>
<p>okay well ...i got 0.0085 also.</p>
<p>i used the R constant in torrs (62.4)</p>
<p>PV/RT = n</p>
<p>(380 torr)(.38L)/(62.4)(273) = 0.0085</p>
<p>barrons is notorious for typos, so yes, the 0.220 should be 0.08206</p>
<p>i've got another ques u know when its a stoic... q they ask for the volume of some gas and they give us the volume of another can i just make them proportional with the coefficients of the gases even if they have the gas at a certain degree and pressure??
sorry if im vague</p>
<p>Yes you can, because the volumes of the gases are proportional to the numbers of moles (at the same condition of temperature and pressure)</p>
<p>i really hate barrons i dont understand anything and they have weird pH log stuff %^&*
i just have one simple question will just studying Sparknotes off of the internet at least guarantee me 600+<br>
im really stuck and i don't have time so i think i should switch what do u guys think from experience?</p>