Ideal Gas Law Help?!?
A mixture of 3.2g H2(g) and 12.0g He(g) in a 4.2-L flask is maintained at 0 degrees celsius. What is the partial pressure of each gas?
A mixture of 3.2g H2(g) and 12.0g He(g) in a 4.2-L flask is maintained at 0 degrees celsius. What is the partial pressure of each gas?
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Verified answer
moles H2 = 3.2 g / 2.016 g/mol=1.6
moles He = 12.0 g / 4.0 g/mol= 3
total moles = 4.6
p = 4.6 x 0.08206 x 273 K/ 4.2 = 24.5 atm
1.6 / 4.6 = partial pressure H2 / 24.5
partial pressure H2 = 8.5 atm
3.0/ 4.6 = partial pressure He/ 24.5
partial pressure He = 16.0 atm