# Problem: Calculate the solubility of O2 in water at a partial pressure of O2 of 120 torr at 25°C. The Henry’s law constant for O2 is 1.3 x 10-3 mol/L • atm for Henry’s law in the form C = kP, where C is the gas concentration (mol/L).

###### FREE Expert Solution

$\overline{){{\mathbf{S}}}_{{\mathbf{gas}}}{\mathbf{=}}{{\mathbf{k}}}_{{\mathbf{H}}}{{\mathbf{P}}}_{{\mathbf{gas}}}}$

where Sgas = solubility of the gas (in mol/L or M), kH = Henry’s law constant for the gas, Pgas = partial pressure of the gas.

92% (250 ratings) ###### Problem Details

Calculate the solubility of O2 in water at a partial pressure of O2 of 120 torr at 25°C. The Henry’s law constant for O2 is 1.3 x 10-3 mol/L • atm for Henry’s law in the form = kP, where C is the gas concentration (mol/L).

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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 Bethel's class at TAMU.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.