<p>I'm posting for my son ... Can somebody explain "torr?" Supposed to calculate how many mL of N2 gas are needed to react completely with lithium metal at 35 C and 771 torr. I told him how smart you guys are. His teacher hasn't mentioned torr but the test is tomorrow.</p>
<p>if i'm not mistaken 1 torr=mL of Mercury above 0... so just convert torrs to atm... which is 771/763... i assume the problem gave the amount of lithium... because you would have to match up the liters of gas to the amount of moles...</p>
<p>1 atmosphere = 760 torr = 760 mm Mercury</p>
<p>if u have it in inches Mercury, convert inches to mm.. look the conversion at a table..</p>
<p>just keep that in mind.. it will help ya..</p>
<p>N2 + 6<em>Li ---> 2</em>Li3N
(i think)</p>
<p>u want to have 6 times less moles of N2 than of N2</p>
<p>u need to know the mass or number of moles originally of lithium</p>
<p>by the way, to determine the number of mls needed.. use the ideal gas law</p>
<p>PV=nRT</p>
<p>Pressure = in atm
Volume = in liters
n = number of moles
R = constant
T = temperature (in kelvin)</p>
<p>im in a hurry right now
ill be able to help u more if u IM me...</p>
<p>My screenname is Variance2004 on AIM</p>
<p>ohhh didn't even think about that... but i thought the actual conversion was 763?*</p>
<p>yup like everyone said: 1 torr= 1 mmHg
771 torr= 771 mmHg
and use PV=nRT to solve
alebed01 looks like he did it right</p>
<p>actually, 760 torr = 1 atm. but the conversion doesn't really matter. torr is just a unit of measuring pressure that's all it is, just like pascals and atms.</p>
<p>dont obsess about the conversions..
understand the concept..</p>