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kH, the Henry's Law constant, for oxygen (O2) in water is 769.2 Latm/mol at 298 degrees K.


Can you help me calculate the solubility and mass based on the following conditions.


kH, the Henry's Law constant, for oxygen (O2) in water is 769.2 Latm/mol at 298 degrees K. Furthermore we know that air at sea level (1 atm.) is 21% oxygen.


I need to calculate the solubility (moles/liter) of O2 in water in these conditions (298 degrees K and 1 atm. total pressure) and  the mass of O2 in grams dissolved in a fishing pond whose volume is 5 x 107 liters when the temperature is 298K and atmospheric pressure of air is 1 atm.

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solubility (moles/liter) of O2 in water is ... View the full answer

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1) Concentration of O 2 =... View the full answer

The mass of O 2 dissolved... View the full answer

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