🤓 Based on our data, we think this question is relevant for Professor Roychowdhury's class at RUTGERS.

The Henry's law constant (k _{H}) for O_{2} in water at 20°C is 1.28 x 10 ^{-3} mol/L•atm. How many grams of O_{2} will dissolve in 1.75 L of H _{2}O in contact with air, where the partial pressure of O_{2} is 1.32 atm?

A. 0.0541 g

B. 0.0473 g

C. 0.0946 g

D. 0.0270 g

E. 0.946 g

We’re being asked to **determine the mass of O _{2}** that will dissolve in

Recall that the solubility of a gas is given by ** Henry’s law**:

$\overline{){{\mathbf{S}}}_{{\mathbf{gas}}}{\mathbf{=}}{{\mathbf{k}}}_{{\mathbf{H}}}{\mathbf{\xb7}}{{\mathbf{P}}}_{{\mathbf{gas}}}}$

where:

**S _{gas}** = solubility of the gas (in mol/L or M)

**k _{H}** = Henry’s law constant for the gas

**P _{gas}** = partial pressure of the gas