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Chapter 11: Q11.3-24E (page 647)

The Henry鈥檚 law constant for \({\bf{O}}_2\)is \({\bf{1}}{\bf{.3 \times 1}}{{\bf{0}}^{{\bf{ - 3}}}}{\bf{ M at}}{{\bf{m}}^{{\bf{ - 1}}}}\)at 25 掳C. What mass of oxygen would be dissolved in a 40 L aquarium at 25 掳C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of \({\bf{O}}_2\)is 0.21 atm?

Short Answer

Expert verified

The mass of oxygen dissolved in a 40-L aquarium at 25 掳C is 0.35g. \(\)

Step by step solution

01

Definition of Henry’s Law

Henry鈥檚 law is a gas law that states that the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid.

02

Explanation

This problem requires the application of Henry鈥檚 law.

The governing equation is:

Cg = kPg

Cg= Concentration of a dissolved gas

k = Henry's Law Constant

Pg= Partial pressure of the gas

Cg = kPg

Cg = 0.0013Matm-1x 0.21atm =2.7 x 10-4molL-1

The total amount =2.7 x 10-4molL x 40L =0.0108mol

The mass of oxygen =0.0108mol x 32gmol-1=0.346g

Mass of Oxygen with two Significant Figures = 0.35g

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