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ozzi
3 years ago
9

The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude. If the solubility of O 2 from the air

is 2.67 × 10 –4 M at sea level and 25°C, what is the solubility of O 2 at an elevation of 12,000 ft where the atmospheric pressure is 0.657 atm?
Assume the temperature is 25°C, and that the mole fraction of O 2 in air is 0.209 at both 12,000 ft and at sea level. 1.75 × 10–4 M 2.67 × 10–4 M 3.66 × 10–5 M 4.06 × 10–4 M
Chemistry
1 answer:
Amiraneli [1.4K]3 years ago
8 0

Answer:

S = 1,75x10⁻⁴M

Explanation:

It is possible to answer this question using Henry's law that states that the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid. The formula is:

S = k×Pi

Where S is solubility, K is Henry's constant and Pi is partial pressure.

At sea level, Pi of O₂ is:

1atm×0,209 = 0,209 atm. Replacing:

2,67x10⁻⁴M = k×0,209atm

k = 1,28x10⁻³M/atm

At 12,000ft Pi of O₂ is:

0,657atm×0,209 = 0,137 atm. Replacing:

S = 1,28x10⁻³M/atm×0,137atm

<em>S = 1,75x10⁻⁴M</em>

<em />

I hope it helps!

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1.- Write the balanced chemical reaction.

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