Problem: Solubilities of four gases in water as a function of temperature. The solubilities are in millimoles per liter of solution, for a constant total pressure of 1 atm in the gas phase.Where would you expect N2 to fit on this graph?

FREE Expert Solution

We have to determine where would the solubility of nitrogen gas (N2) lie on the given solubility-temperature curve.


The solubility of a gas in water is affected by various factors such as:

  • Polarity of the gas
  • Partial pressure of gas
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Problem Details

The x-axis is temperature in degrees C, ranging from 0 to 50 with intervals of 10. The y-axis is solubility (millimoles), ranging from 0 to 2.0 with intervals of 1.0.  Methane is 2.25 mmol at 4 C, 1.80 at 10 C, 1.50 at 20 C, 1.25 at 30 C, and 1.10 at 40 C. Diatomic oxygen is 1.90 mmol at 4 C, 1.70 at 10 C, 1.30 at 20 C, 1.20 at 30 C, and 1.00 at 40 C. Carbon monoxide is 1.40 mmol at 4 C, 1.25 at 10 C, 1.10 at 20 C, 0.85 at 30 C, and 0.76 at 40 C. Helium is 0.50 mmol at 4 C, 0.45 at 10 C, 0.45 at 20 C, 0.35 at 30 C, and 0.35 at 40 C.
Solubilities of four gases in water as a function of temperature. The solubilities are in millimoles per liter of solution, for a constant total pressure of 1 atm in the gas phase.

Where would you expect N2 to fit on this graph?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Henry's Law concept. You can view video lessons to learn Henry's Law. Or if you need more Henry's Law practice, you can also practice Henry's Law practice problems.