1,324ACalculate the masses of oxygen and nitrogen that aredissolved in 1.5 L of aqueous solution in equilibrium with airat 25 °C and 760 Torr. Assume that air is 21% oxygen and78% nitrogen by volume.mass:FEB22~tvmg 0₂MacBook ProHenry's law constants for gases in water at25 °Cmass:GasHeN₂0₂CO2H₂SA Okh (bar - M-¹)2.7 x 10³1.6 × 10³7.9 x 10²2910.Wmg

Answered: Calculate the masses of oxygen and…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.106QE: In the 1986 Lake Nyos disaster (see the chapter introduction), an estimated 90 billion kilograms of...

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1,324
A
Calculate the masses of oxygen and nitrogen that are
dissolved in 1.5 L of aqueous solution in equilibrium with air
at 25 °C and 760 Torr. Assume that air is 21% oxygen and
78% nitrogen by volume.
mass:
FEB
22
~
tv
mg 0₂
MacBook Pro
Henry's law constants for gases in water at
25 °C
mass:
Gas
He
N₂
0₂
CO2
H₂S
A O
kh (bar - M-¹)
2.7 x 10³
1.6 × 10³
7.9 x 10²
29
10.
W
mg

Expert Solution

Step 1

To solve this problem, we will use Henry's law, which relates the partial pressure of a gas above a liquid to the concentration of the gas dissolved in the liquid. The equation is:

P_gas = k_h * [gas]

where P_gas is the partial pressure of the gas above the liquid, [gas] is the concentration of the gas dissolved in the liquid, and k_h is the Henry's law constant for the gas at a given temperature.

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