(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

The activity coefficient of zinc in liquid brass is given (in joules) by the following equation for

temperatures 1000-1500 K:

RT ln γZn = -38,300 x2Cu

where xCu is the mole fraction of copper. Calculate the partial pressure of pure zinc PZn over a

solution of 60 mol% copper and 40 mol % zinc at 1200 K. The vapor pressure of pure zinc is

1.17 atm at 1200 K.

2. Relevant equations

For dilute solutions: xs: mole fraction of solvent, xu: mole fraction of solute,

The vapour pressure of the solvent= Ps= P(pure)xs=P(pure)(1-xu) where is P(pure)=vapour pressure of the pure solvent.

Gibbs-Duhem Relationship=

lnaB

lnaA= - ∫ xB/ xa * d(lnaB)

-∞

3. The attempt at a solution

d (lnγA)= - XB/XA * d(lnγB) applying Gibbs-Duhem rel. in the form of this eqnn:

dxcu= -dXzn

lnγCu= - 38.300/ RT * X^2Zn

How can i get the partial pressure of pure zinc PZn?

Thanks! :)

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# Calculating the partial pressure of pure Zinc over a solution? over

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