Verified answer

After John Dalton behaves each gas component in a gas compound as when it would exist alone.

That means you can apply the general gas equation:

pV=mRT

N compounds give you N equations:

You have 2 components --->N=2

p1*V=m1*R1*T

p2*V=m2*R2*T

p1,2=partial pressures of the components 1(He) and 2(Xe)

V=Volume

m1,2=masses 1(He) and 2(Xe)

R1,2=Gas constants 1(He) and 2(Xe)

T=absolute temperature

p1=mi*Ri*T/V

with

T/V = p/mR

p1 = [(m1*R1)/(m*R)]*p

mu1 = m1/m = n1*M1/(n*M) =r1*M1/M

mu1=ratio mass (He) / total mass

n1=amount of substance or mole number (He)

M1=Mole mass (He)

M=Mole mass compound

r1= mole fraction

you get

p1=[(m1*R1)/(m*R)]*p = mu1*(R1/R)*p

with r1=V1/V

p1=r1*p=(V1/V)*p

-------------------------

p2=r2*p=(V2/V)*p

-------------------------

The gases are 50% each by mass.

Work out what they are by volume. That will then give you the effective partial pressures. I do not have a calculator, but if volume of He was 3 and of Xe was 3 then the partial; pressure of He would be 3/(3+2) X 600 Torr