Question

Calculate the partial pressure and gas-phase concentration (in ppm) of n-octane in air when the air is saturated with that VOC. The total pressure is 1 atm and the temperature is 100ºC.

Answer #1

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.

Suppose 0.420 kg of octane (C8H18) is burned in air at a
pressure of 1 atm and temperature of 20°C, what volume of carbon
dioxide gas is produced?

Calculate the mole fraction of ethane
(C2H6) in water at 10ºC when the ethane
concentration in air that is in equilibrium with the water is
10,000 ppm. The total pressure is 5.0 atm.

Concentration of a gas is 0.75 M in water at 25C when the
pressure of the gas over the solution is 3.5 atm. What is the
Henry's law constant for this gas in water at that temperature?

A solution contains 49.0 g of heptane (C7H16)and 59.0 g of
octane (C8H18) at 25 ∘C. The vapor pressures of pure heptane and
pure octane at 25 ∘C are 45.8 torr and 10.9 torr, respectively.
Assuming ideal behavior, calculate each of the following. (Note
that the mole fraction of an individual gas component in an ideal
gas mixture can be expressed in terms of the component's partial
pressure.)
A) The vapor pressure of heptane in the mixture
B) The Vapor...

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...

Calculate the partial pressure, in atmospheres, of O2
in the dry air outside an airliner cruising at an altitude of about
30000 ft (9144 m), where the atmoshperic pressure is 231 mm Hg. How
much must the outside air be compressed to produce a cabin pressure
in which the partial pressure of O2 is 0.200 atm?

Calculate the concentration of Co2 in rainwater at 25C using
Henry's law. Assume that the water is saturated with air that
contains 350 ppm of CO2. The Henry's law constant for CO2 is
KH=3.4X10-2 MOL/L-ATM at 15C . Express the result in molarity and
ppm. Calculate the concentration of NO in rainwater at 25 C that is
in equlibrium with polluted air where the NO concentration is 10
ppm. The Henry's law constant for No is Kh=2x10-4 mol/l-atm at 25C...

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