Question

Given that the vapor pressure of water is 17.54 Torr at 20 °C, calculate the vapor-pressure lowering of aqueous solutions that are 2.40 m in (a) sucrose, C12H22O11, and (b) calcium chloride. Assume 100% dissociation for electrolytes.

Answer #1

Sucrose: i = 1. mc = m*i = 2.4 * 1 = 2.4

CaCl2: i = 3. mc = 2.4 * 3 = 7.2

2. Calculate the moles of water.

Assume there are 1000g of water.

1000 g H2O * (1 mol / 18 g) = 55.5 moles of H2O

3. Calculate the mole fraction of each.

Sucrose: X = 2.4 mol / (2.4 + 55.5 mol) = 0.04145

CaCl2: X = 7.2 mol / (7.2 + 55.5 mol) = 0.11483

4. Calculate the vapor pressure lowering using Raoult's Law: ΔP =
X*P°.

**Sucrose: ΔP = (0.04145)(17.54 Torr) = 0.7270 Torr
CaCl2: ΔP = (0.11483)(17.54 Torr) = 2.0141 Torr**

Given that the vapor pressure of water is 17.54 Torr at 20 °C,
calculate the vapor-pressure lowering of aqueous solutions that are
2.10 m in (a) sucrose, C12H22O11, and (b) calcium chloride. Assume
100% dissociation for electrolytes.

Given that the vapor pressure of water is 17.54 Torr at 20 °C,
calculate the vapor-pressure lowering of aqueous solutions that are
1.90 m in (a) sucrose, C12H22O11, and (b) calcium chloride. Assume
100% dissociation for electrolytes.

1) What will the solution vapor pressure be for a solution of
11.07 mol of sucrose (C12H22O11)
dissolved in 1.000L of water at 20.0 °C? The vapor pressure of pure
water at 20.0 °C is 17.5 torr. (Show work)
2) Calculate the freezing point of a solution containing 0.43 of
sucrose in 150 mL of water. Kf = 1.86 °C/m (Show
Work)

1. A solution of sodium chloride in water has a vapor pressure
of 19.6 torr at 25ºC. What is the mole fraction of solute particles
in this solution? What would be the vapor pressure of this solution
at 45ºC? The vapor pressure of pure water is 23.8 torr at 25ºC and
71.9 torr at 45ºC, and assume sodium chloride exists as Na+ and Cl-
ions in solution.

Physical chemistry
The vapor pressure of water is 760 torr at 100 °C and 100 torr
at 51.6 °C. Estimate the molar heat of vaporization (delta Hvap,m)
at the midpoint of this temperature range, and delta Hvap,m
at room temperature assuming delta
Cp,m = - 41.5 J/K.mol

At 20 ∘C the vapor pressure of benzene C6H6 is 75 torr and that
of toluene C7H8 is 22 torr. Assume that benzene and toluene form an
ideal solution.
a) In a solution composed of benzene and toluene that has a
vapor pressure of 37 torr at 20 ∘C, what is the mole fraction of
benzene?
b) In a solution composed of benzene and toluene that has a
vapor pressure of 37 torr at 20 ∘C, what is the mole...

25g
glucose (C6H12O6) is mixed with 90g water and dissolved. Calculate
the vapor pressure of the solution. The vapor pressure for water is
17.54 torr.
(On the answer sheet my teacher has 17.1torr but doesnt have
how he got that)

The vapor pressure of water at 25°C is 23.8 torr, and the heat
of vaporization of water at 25°C is 43.9 kJ/mol. Calculate the
vapor pressure of water at 65°C. PLEASE CAN YOU SHOW A
STEP-BY-STEP?

The vapor pressure of pure water at 25.0 oC is 23.8 torr. What
is the vapor pressure (at 25.0 oC), in atm, of an aqueous solution
of 54.0 g glucose (C6H12O6), MM = 180. g mol-1) in 285.0 g of
water? 760 torr = 1 atm P1 = X1Po1 Circle your choice.
a) 0.0451 b) 0.194 c) 0.0307 d) 0.105 e) 0.146 f) 0.0287

At 20 ∘C the vapor pressure of benzene (C6H6) is 75 torr, and
that of toluene (C7H8) is 22 torr. Assume that benzene and toluene
form an ideal solution. What is the mole fraction of benzene in the
vapor above the solution described in part (a)? 39 torr at 25 C

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 5 minutes ago

asked 8 minutes ago

asked 8 minutes ago

asked 18 minutes ago

asked 19 minutes ago

asked 26 minutes ago

asked 32 minutes ago

asked 35 minutes ago

asked 35 minutes ago

asked 38 minutes ago

asked 39 minutes ago

asked 41 minutes ago