use ideal gas equation to find initially pressure without N2O4 PV = nRT { P = pr

Question

use ideal gas equation to find initially pressure without N2O4

PV = nRT

{ P = pressure in atm, V = volume in L, n = no. moles of NO2, R = ideal gas constant = 0.082 atm L / K mol and T = temperature in K}   

first find moles of NO2 = mass / molar mass = (7.18 g / 46.0 g/mol) = 0.156 moles

P = nRT / V

P = [ (0.156 moles) x (0.082 L atm / K mol) x (300 K ) ] / 3.5 L

P = 1.096 atm

final pressure of closed container = 0.75 atm

partial pressure of one individual gas

Pi = Ptotal X

{ X = mole fraction }

1.096 atm = 0.75 atm x X

X = 1.46133

NO2 / N2O4 = 1.46133

NO2 = 0.40

N2O4 = 0.60

Explanation / Answer

up dr VIID o points) Nitrogen dioxide dimerizes to give dinitrogen tetroxide. Page 7 of S 2 NO2(g) N3O4(g) At 300 K, initially, 7.18 g of NO2 (no N204) is added into a 3.50-L closed container. A.fter a certain period, the pressure of the closed container is measured to be 0.75 atm. What are the mole fractions of the two gases in the NO2/N2O4 mixture? (Hint: Initially, the system contains only NO2. After a certain period, the system contains a mixture of NO2/N204.)

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