A vessel containing Ne(g) and Ar(g) has a total pressure of 9.78. If the partial pressure of the Neon (PNe) is 3.78 and the partial pressure of the Argon (PAr) is 6, then the mole-fraction of Ne(g) is _ and the mole-fraction of Ar(g) is __.

According to the Dalton's Law, the partial pressure exerted by component 'i' in a gas mixture is equal to the product of the mole fraction of the component and the total pressure.

Formula used :

[tex]p_i=X_i\times p_T[/tex]

where,

[tex]p_i[/tex] = partial pressure of gas

[tex]X_i[/tex] = mole fraction of gas

[tex]p_T[/tex] = total pressure of gas

Now we have to determine the partial pressure of [tex]Ne[/tex] and [tex]Ar[/tex]

[tex]p_{Ne}=X_{Ne}\times p_T[/tex]

Given:

[tex]p_{Ne}=3.78\\\\p_T=9.78[/tex]

[tex]3.78=X_{Ne}\times 9.78[/tex]

[tex]X_{Ne}=0.387[/tex]

and,

[tex]p_{Ar}=X_{Ar}\times p_T[/tex]

Given:

[tex]p_{Ar}=6\\\\p_T=9.78[/tex]

[tex]6=X_{Ar}\times 9.78[/tex]

[tex]X_{Ar}=0.613[/tex]

Therefore, the mole fraction of [tex]Ne[/tex] and [tex]Ar[/tex] is, 0.387 and 0.613 respectively.

A vessel containing Ne(g) and Ar(g) has a total pressure of 9.78. If the partial pressure of the Neon (PNe) is 3.78 and the partial pressure of the Argon (PAr) is 6, then the mole-fraction of Ne(g) is _______ and the mole-fraction of Ar(g) is ________.

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A vessel containing Ne(g) and Ar(g) has a total pressure of 9.78. If the partial pressure of the Neon (PNe) is 3.78 and the partial pressure of the Argon (PAr) is 6, then the mole-fraction of Ne(g) is _ and the mole-fraction of Ar(g) is __.