Question
Asked Oct 15, 2019
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A 355 cm^3 sample of air saturated with water vapor at 27 degrees celsius generates a total pressure of 775 mmHg. How many grams of O2 are present in the sample, given that water has a vapor pressure of 26.7 mmHg and air can be assumed to be 20% O2 and 80% N2?

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Expert Answer

Step 1

The number of moles for a given chemical species refers to the ratio of mass to the molar mass. The mathematical formula which is used to calculate the number of moles is as follows:

Mass
Number of moles=.
Molar mass
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Mass Number of moles=. Molar mass

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Step 2

The ideal gas law which is also known as the equation of state is an equation of state of a hypothetical ideal gas. The equation can be written as follows:

PV=nRT
P is the pressure of the gas
V is the volume of the gas
n is the number of moles
T is the temerpatyure of the system
R is the gas constant
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PV=nRT P is the pressure of the gas V is the volume of the gas n is the number of moles T is the temerpatyure of the system R is the gas constant

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Step 3

The volume of the sample of the air is given to be 355 cm3=0.355 L.

T=27oC=300.15 K

Ptotal=775 mmHg

Pwater= 26.7 mmHg

...
Р. -Ро, "Ру, -Рно
775 mmHg Po,+P,)+ 26.7 mmHg
P -(Ро, +Ру, )-775 mmHg -26.7 mmHg
Р. -748.3 mmHg
air
air
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Р. -Ро, "Ру, -Рно 775 mmHg Po,+P,)+ 26.7 mmHg P -(Ро, +Ру, )-775 mmHg -26.7 mmHg Р. -748.3 mmHg air air

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