PLS HELP "NO LINKS" Given that the mass density of air at 0.987 bar and 27°C is 1.146 kg·m−3, calculate the mole fraction and partial pressure of nitrogen and oxygen assuming the following conditions.
(a) air consists only of these two gases
mole fraction nitrogen:

mole fraction oxygen:

partial pressure nitrogen:

partial pressure oxygen:

(b) air also contains 1.0-mole percent Ar
mole fraction nitrogen:

mole fraction oxygen:

partial pressure nitrogen:

partial pressure oxygen:

partial pressure argon:

All answers need to be in sig fig 4
Thanks!

pv=nrt

explanation:

a. the law of proportion states the combination of 2 atoms in a specific ratio to produce multiple compounds such as the given statement of question ‘1st compound contains 88.8 % cu ’ indicates 88.8 g of cu is present along with 11.2 g oxygen in 100 g of compound whereas the statement ‘2st compound contains 79.9 % cu ’ indicates 79.9 g of cu is present along with 20.1 g oxygen in 100 g of compound

1st compound contains 88.8 g cu

for cu

m = 63 g /mol

atomic % = 88.8 /63 = 1.42

for o

m = 16 g /mol

atomic % = 11.2 /16 = 0.7

b. the emperical formula of 1st compound is

cu1.4o0.7

cu2o