Tricky Chemistry questions - answered by ChemTutor.me
Question:
Sample of dry gas 25c has the
following composition 0.8904g of N2 0.2741g of O2 0.0152g of Ar 0.00107g of CO2
R=0.0821 What are the partial pressure for each component in the mixture?? what
is the total pressure??
Answer:
Calculate the number of moles of each gas in
mixture:
n(N2) = m(N2)/M(N2) =
0.8904/(14.007∙2) = 0.0317841 mol n(O2) = m(O2)/M(O2) =
0.2741/(15.999∙2) = 0.0085662 mol n(Ar) = m(Ar)/M(Ar) = 0.0152/39.948 =
0.0003805 mol
n(CO2) =
m(CO2)/M(CO2) = 0.00107/(12 + 15.999∙2)
= 0.0000243 mol
The total
pressure of mixture cannot be found from the provided data. We can assume that
the pressure of mixture is atmospheric. Hence we can calculate the partial
pressure of each component in mixture.
n(total) = 0.31784 + 0.008566 + 0.0003805 +
0.0000243 = 0.040755 mol
x(N2) =
n(N2)/n(total) = 0.7799
x(O2) =
n(O2)/n(total) = 0.2102
x(Ar) = n(Ar)/n(total) = 0.00934
x(CO2) =
n(CO2)/n(total) = 0.000596
pi = xi∙p(total)
p(N2) = n(N2)/n(total)
= 0.7799∙101325 Pa = 79020 Pa p(O2) = n(O2)/n(total)
= 0.2102∙101325 Pa = 21300 Pa p(Ar) = n(Ar)/n(total) = 0.00934∙101325 Pa = 946
Pa
p(CO2) =
n(CO2)/n(total) = 0.000596∙101325
Pa = 60.4 Pa
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