Question

At 20^{o}C, the partial pressure of water is 0.0231 atm,
meaning water vapor accounts for _____% of the air.

Answer #1

air pressure = 1 atm

water pressure = 0.0231

water vapor pressure percentage = water pressure x 100 / total air pressure

= 0.0231 x 100 / 1

**
= 2.31 %**

The vapor pressure of benzene is 9959 Pa at 20oC, and the vapor
pressure of toluene is 2973 Pa at 20 oC. A certain solution of
benzene and toluene at 20oC has a vapor pressure of 6133 Pa. Find
the benzene mole fraction in this solution and in the vapor above
this solution.

Air is dried from a partial pressure of 50 mm Hg of water vapor
to a partial pressure of 10 mm Hg. The temperature of the entering
air is 524°F and the pressure is constant at 760 mm Hg. How many
gallons of liquid water are removed per 1000 ft3 of entering
air?

Calculate the partial pressure and gas-phase mole fraction of NO
in air that is in contact with water that has a mole fraction of
1.0(10)-6 NO. The temperature and pressure are
20oC and 1 atm.

The vapor pressure of a solvent at 20oC is 17.5 Torr. The vapor
pressure decreases by 0.62 Torr when 800 grams of this solvent is
thrown out of some salt. According to this;
(A) The vapor pressure of the solution
(B) Mole fraction of solvent
(C) Calculate the molality of the salt (Mole weight of solvent =
18 g / mol)
(D) If the freezing point lowering of the solution is 0.66, find
the cryoscopy constant of the solvent.

the solubility of N2 in blood at 37C and at a partial pressure
of 0.80 atm is 5.6x10-4 mol/L a deep sea diver breathes compressed
air with the partial pressure of N2 equal to 3.5atm assume that the
total volume of blood is5.8L Calculate the amount of n2 gas
released(in liters at 37 degree C and 1.00atm) when the diver
returns to the surface of the water where the partial pressure of
N2 is 0.80 atm

The solubility of N2 in
blood at 37°C and at a partial pressure of 0.80
atm is5.6 × 10−4 mol/L. A deep-sea
diver breathes compressed air with the partial pressure of
N2 equal to 5.0 atm. Assume that the
total volume of blood in the body is 5.2 L. Calculate the amount of
N2 gas released (in liters at
37°C and 1.00 atm) when the diver returns to the
surface of the water, where the partial pressure of
N2 is...

The solubility of N2 in blood at 37°C and at a partial pressure
of 0.80 atm is 5.6 × 10−4 mol/L. A deep-sea diver breathes
compressed air with the partial pressure of N2 equal to 4.5 atm.
Assume that the total volume of blood in the body is 5.2 L.
Calculate the amount of N2 gas released (in liters at 37°C and 1.00
atm) when the diver returns to the surface of the water, where the
partial pressure of N2...

The relative humidity of air equals the ratio of the partial
pressure of water in the air to the equilibrium vapor pressure of
water at the same temperature times 100%. If the relative humidity
of the air is 58% and its temperature is 68 oF , how many moles of
water are present in a room measuring 12 ft x 10 ft x 8 ft? The
vapor pressure of water at 68 oF is 17.54 torr. The answer is 20,...

The vapor pressure of pure liquid water is p*(H2O) = 0.02308
atm. Above an aqueous solution with 122 g of a non-volatile solute
(molar mass 241 g/mol) in 920 g H2O has a vapor pressure of 0.02239
atm. Calculate the activity and the activity coefficient of water
in the solution.

What is the vapor pressure in atm of a solution at 25
oC produced by dissolving 120.1 g of dextrose
(C6H12O6) in 395.2 g of water?
Vapor pressure of water at 25 oC = 0.0313 atm

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