Question

oxygen is bubbled through water at 293K assuming that oxygen exerts a partial pressure of 0.98 bar, the solubility of oxygen in g/ml is ??? given Henry's law constant is 34K bar ​

Answer 1

Answer:

The solubility of the oxygen gas is 0.05 g/L.

Explanation:

Partial pressure of the oxygen gas,$$p__{O_2}$$ = 0.98 bar

Henry's Law constant $$K_H$$ for oxygen gas = 34.84 kbar = 34840 bar

$$p_{O_2}=K_H\times \chi_{O_2}$$

$$\chi_{O_2}=\frac{0.98 bar}{34840 bar}=2.81\times 10^{-5}$$

$$\chi_w=0.9999$$

Moles of water = 0.999

Mass of water = $$18 g/mol\times 0.999 mol=17.98 g$$

Density of water = 1000 g/L

Volume of water =$$\frac{17.98 g}{1000 g/L}=0.01798 L$$

Moles of oxygen gas = $$2.81\times 10^{-5}$$

Mass of oxygen gas = $$32\times g/mol\times 2.81\times 10^{-5}=89.92\times 10^{-5} g$$

Solubility of oxygen gas:$$\frac{89.92\times 10^{-5} g}{0.01798 L}=0.05 g/L$$

The solubility of the oxygen gas is 0.05 g/L.