Question #655b9
2 Answers
Answer will be (2) 140 mm of Hg .
Explanation:
We have , A + B -------> AB
Mole fraction (X) of A = 0.8 ; X of B will be = 1 - 0.8 = 0.2
Now , we are given , V.P and of pure A and V.P of solution AB as 70 and 84 mm of Hg respectively .
As it forms an ideal solution , therefore ;
V.P of AB = Partial V.P of A + Partial V.P of B
Partial V.P of any component = X of that component * V.P of that component in pure state
Therefore , substituting the values in
V.P of AB = Partial V.P of A + Partial V.P of B ; we get ,
84 = 70 * 0.8 + V.P of pure B * 0.2
Solving this we get 140 mm of Hg as the V.P of pure B .
I get
The temperature is just for context.
This question is basically asking you to use Raoult's law for ideal binary mixtures:
#\mathbf(P_j = chi_jP_j^"*")# where:
#P_j# is the "non-pure" vapor pressure of the solution (i.e. when there is component#i# in it).#P_j^"*"# is the vapor pressure of the pure component j (i.e. the solution with no component#i# ).#chi_j# is the#\mathbf("mol")# fraction of component#j# in solution. As#chi_j -> 1# ,#P_j -> P_j^"*"# .
You have:
#P_A^"*" = "70 mm Hg"# #chi_A = 0.8# #P_"tot" = "84 mm Hg"# #P_B^"*" = ?#
in an ideal binary mixture of
#\mathbf(P_"tot" = P_A + P_B)#
Now, combine this with Raoult's law (best for ideal binary mixtures!) to get:
#P_"tot" = chi_AP_A^"*" + chi_BP_B^"*"#
Here we can use the fact that
#color(blue)(P_"tot") = chi_AP_A^"*" + (1 - chi_A)P_B^"*"#
#= chi_AP_A^"*" + P_B^"*" - chi_AP_B^"*"#
Now you can solve for
#P_"tot" - chi_AP_A^"*" = P_B^"*"(1 - chi_A)#
#color(blue)(P_B^"*") = (P_"tot" - chi_AP_A^"*")/(1 - chi_A)#
#= (84 - 0.8*(70))/(1 - 0.8)#
#= (84 - 56)/(0.2)#
#= 28*5 = color(blue)("140 mm Hg")#