Question

A gaseous mixture contains 449.0 Torr H2(g), 327.5 Torr N2(g), and 89.5 Torr Ar(g). Calculate the mole fraction, , of each of these gases.

Answer 1

XH2 = 0.5185; XN2 = 0.3782; XAr = 0.103

Step-by-step explanation:

Let's say the mole fraction is Xi, i is individual gas, and Pi is partial pressure.

`X_i=(P_i)/(P_(total))`

Ptotal is all the pressure added together, which is:

449.0torrH2 + 327.5torrN2 + 89.5torrAr = 866.0torr

From this point, it's pretty simple, just plug the values into the equation (watch out sig figs):

XH2 = 449.0torr/866.0torr = 0.5185
XN2 = 327.5torr/866.0torr = 0.3782
XAr = 89.5torr/866.0torr = 0.103