Question

A solution is prepared by adding 1.50 mol glucose, which is not volatile, to 3.50 mol water. What is the vapor pressure of this solution at 25 C given that the vapor pressure of pure water is 23.8 torr?

Answer #1

Mole fraction of water in glucose solution can be calculated as follows:

Mole fraction of water = moles of water/(total moles of glucose and water)

Mole fraction of water = 3.50 mol / (1.50 + 3.50) mol

Mole fraction of water = 0.700

Vapor pressure of glucose solution can be calculated by using Raoult’s Law expression as follows:

Vapor pressure = Vapor pressure of pure water x mole fraction of water

Vapor pressure = 23.8 torr x 0.700

Vapor pressure = 16.7 torr

Therefore, vapor pressure of glucose solution is **16.7 torr**.

What is the vapor pressure of the solution that contains 25g of
mannose (non-volatile non-electrolyte MW 180.16 g/mol) and 75g of
water (MW 18)? The vapor pressure of pure water is 23.8 torr.
I know the answer is 23, but I do not know how to get it.

Part A. If 0.680 mol of a nonvolatile nonelectrolyte are
dissolved in 3.90 mol of water, what is the vapor pressure PH2O of
the resulting solution? The vapor pressure of pure water is 23.8
torr at 25 ∘C .
Part B. A solution is composed of 1.00 mol cyclohexane
(P∘cy=97.6 torr) and 2.50 mol acetone (P∘ac=229.5
torr). What is the total vapor pressure Ptotal above this
solution?

Part A
If 0.560 mol of a nonvolatile nonelectrolyte are
dissolved in 3.40 mol of water, what is the vapor pressure
PH2O of the resulting solution? The vapor pressure of pure
water is 23.8 torr at 25 ∘C .
Part B
A solution is composed of 1.90 mol cyclohexane
(P∘cy=97.6 torr) and 2.80 mol acetone (P∘ac=229.5
torr). What is the total vapor pressure Ptotal above this
solution?

1) Consider two solutions, one formed by adding 10 g of glucose
to 1L of water and the other formed by adding 10g of sucrose to 1L
of water. Calculate the vapor pressure for each solution at 20oZC;
the vapor pressure of pure water at this temperature is 17.5
torr.

the vapor pressure of water at 25°c is 23.8 torr.
determine the mass of glucose(molar mass =180g/mol) needed to add
to 500g water to change the vapor pressure to 23.1 torr.

A solution is made by dissolving 24.1 g urea (), a
nonelectrolyte, in 309 g water. (The vapor pressure of pure water
is 23.8 torr at 25°C and 71.9 torr at 45°C.)
Calculate the vapor pressure of this solution at 25°C.
Vapor pressure = torr
Calculate the vapor pressure of this solution at 45°C.
Vapor pressure = torr

An aqueous solution is formed by dissolving 8.00 mol of a
non-electrolyte in 1.00 kg of water. If the vapor pressure of pure
water is 23.8 mm Hg at 25/C, the vapor pressure of the solution
will be:
19.4 mm Hg
23.8 mm Hg
5.5 mm Hg
26.8 mm Hg
20.8 mm Hg

A solution is prepared by dissolving 88.5g of sugar, C6H12O6, in
300ml of water. What is the vapor pressure of the solution? Vapor
pressure of pure water is 28 torr at that temperature.

10. A solution contains 6.50 mol water, 0.300 mol sucrose, and
0.200 mol glucose. The solutes are nonvolatile. What is the vapor
pressure of the solution at 35°C given that the vapor pressure of
water is 42.2 torr?
35.0 torr d. 39.2 torr
36.0 torr e. 39.0 torr
37.0 torr
11. Indicate which aqueous solution has the fastest evaporation
rate.
0.1 M KCl d. 0.1 M MgCl2
0.2 M Na2CO3 e. 0.2 M MgCl2
0.2 M NaCl
12. Identify the...

what is the vapor pressure of a solution containing 0.500 mol
of glucose and 5.000 mol of water at 29 degrees C?

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