<h3><u>Answer;</u></h3>
- <u>0.433 g N2 </u>
- <u>0.293 g O2 </u>
- <u>0.0367 g He</u>
<h3><em>Explanation and solution;</em></h3>
- We can start by getting the total pressure; which will be the sum of the partial pressure of each gas.
221 torr + 131 torr + 131 torr
P (total) = 483 torr total
n = PV / RT, we can determine the total number of moles of the mixture
= (483 torr) x (1.30 L) / ((62.36367 L Torr/K mol) x (25.0 + 273.15 K))
= 0.033769 mol gases total
-
Therefore; we can determine the mass of each gas;
- <u>Nitrogen gas </u>
<em>N2 = 28.01 g/mol</em>
<em>= (0.033769 mol) x ( 221 torr N2/ 483 torr) x (28.01 g N2/mol) </em>
<u>= 0.433 g N2 </u>
<em>
O2 = 32 g/ mol </em>
<em> =(0.033769 mol) x (131 torr O2/ 483 torr) x (32 g O2/mol)</em>
<em> </em><em><u>= 0.293 g O2 </u></em>
- <em><u>Helium gas </u></em>
<em><u>
</u></em><em>He = 4 g/mol</em>
<em>= (0.033769 mol) x (131 torr He/ 483 torr) x (4.00 g He/mol) </em>
<em><u>= 0.0367 g He</u></em>