Answer :
The vapour pressure of the solution exists 83.24 mmHg.
How to find the vapour pressure of the solution?
The vapor pressure of the solution
(Psolution) = (Xmethanol)(P°methanol).
where Psolution exists the vapor pressure of the solution,
Xmethanol exists as the mole fraction of methanol,
P°methanol exists in the pure vapor pressure of methanol.
We must estimate the mole fraction of methanol (Xmethanol).
Xmethanol = (n)methanol/(n) total.
where n methanol exists the number of moles of methanol.
n total exists the total number of moles of methanol and urea.
We can estimate the number of moles of both methanol and urea utilizing the relation: n = mass/molar mass.
n of methanol = mass/molar mass = (56.9 g)/(32.04 g/mol) = 1.776 mol.
n of urea = mass/molar mass = (7.38 g )/(60.06 g/mol) = 0.123 mol.
∴ Xmethanol = (n)methanol/(n) total
= (1.776 mol)/(1.776 mol + 0.123 mol) = 0.935.
∴ Psolution = (Xmethanol)(P°methanol)
= (0.935)(89.0 mmHg) = 83.24 mmHg.
The complete question is:
What is the vapor pressure at 20 °c of an ideal solution prepared by the addition of 7.38 g of the nonvolatile solute urea, co(nh2)2, to 56.9 g of methanol, ch3oh? the vapor pressure of pure methanol at 20 °c is 89.0 mm hg.
To learn more about ideal solutions refer to:
https://brainly.com/question/17071556
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