What would be the saturation concentration (mole/L) of oxygen (O2) in a river in winter when the air temperature is 0°C if the Henry's law constant at this temperature is 2.28 * 10-3 mole/L-atm? What would the answer be in units of mg/L?

Question

Chemistry

Libby

4 April, 15:43

What would be the saturation concentration (mole/L) of oxygen (O2) in a river in winter when the air temperature is 0°C if the Henry's law constant at this temperature is 2.28 * 10-3 mole/L-atm? What would the answer be in units of mg/L?

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Answers (1)

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Cheyenne Hicks · Answer 1

20.21*10^-4 mg/L is the concentration.

Explanation:

Given:

Pressure=1 atm.

Temperature = 0 degrees

Volume percent of air is 21%

Henry's Law constant K = 2.28 x 10^-3 mole/L-atm

The partial pressure of oxygen is 0.21 atm.

By Henry's law:

Concentration = K X Partial pressure

= 2.28*10^-3 * 0.21

= 4.79*10^-4 moles/litre

Since, at STP 1 mole of oxygen occupies volume of 22.4L

concentration = mass/volume

mass = 4.79*10^-4-4*22.4

= 20.21*10^-4 mg

20.21*10^-4 mg/L is the concentration.