Question

Henry Law’s Constants at a system temperature of 25°C (77°F) of oxygen is 756.7 atm/(mol/litre). Molar Weight of O2 is 31.9988 g/mol and partial fraction in air is ~ 0.21. Calculate the Oxygen dissolved in the Water at atmospheric pressure.

(a) 0.0090 g/liter

(b) 0.0089 g/liter

(c) 0.0080 g/liter

(d) 0.0099 g/liter

This question was addressed to me in quiz.

This intriguing question originated from Estimating Oxygen Solubility in division Mass Transfer of Bioprocess Engineering

Answer 1

The correct choice is (b) 0.0089 g/liter

Easiest explanation: Oxygen dissolved in the Water at atmospheric pressure can be calculated as:

c = pg / kH

co = (1 atm) 0.21 / (756.7 atm/(mol/litre)) (31.9988 g/mol)

= 0.0089 g/liter.