What is the mass of oxygen dissolved in a 7.0L fish tank when pressure of air...

What is the mass of oxygen dissolved in a 7.0L fish tank when pressure of air is 0.98atm and the mole fraction of oxygen in air is 0.22. T=25 C degrees, Henry's constant KH for O2 is 1.3 x 10^-3 M/atm at 25 C degrees.
A) 62.9 mg
B) 123.6 mg
C) 48.9 mg
D) 285.4 mg

Expert Solution

partial pressure of O2 = total pressure x mole fraction

= 0.98 x 0.22

= 0.2156 atm

molarity of O2 = KH x partial pressure

= 1.3 x 10^-3 x 0.2156

= 2.8028 x 10^-4 M

moles = molarity x volume

= 2.8028 x 10^-4 x 7.0

= 1.96 x 10^-3

mass of O2 = 1.96 x 10^-3 x molar mass

= 1.96 x 10^-3 x 32

= 0.0629 g

= 62.9 mg

answer : A) 62.9 mg

queen_honey_blossom answered 2 years ago

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