Problem: The Henry’s law constant for O2 is 1.3 × 10−3 M/atm at 25 °C. What mass of oxygen would be dissolved in a 40-L aquarium at 25 °C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of O2 is 0.21 atm?

🤓 Based on our data, we think this question is relevant for Professor Petros' class at UNT.

FREE Expert Solution

(1) Calculate the molar solubility of the O2

Sgas = KH×PgasSgas = (1.3x10-3 Matm)(0.21 atm)

Sgas = 2.73x10-4 M

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Problem Details

The Henry’s law constant for Ois 1.3 × 10−3 M/atm at 25 °C. What mass of oxygen would be dissolved in a 40-L aquarium at 25 °C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of O2 is 0.21 atm?

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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.

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Based on our data, we think this problem is relevant for Professor Petros' class at UNT.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.