   Chapter 13, Problem 23PS

Chapter
Section
Textbook Problem

A sealed flask contains water and oxygen gas at 25 °C. The O2 gas has a partial pressure of 1.5 atm. (a) What is the concentration of O2 in the water? (b) If the pressure of O2 in the flask is raised to 1.7 atm, what happens to the amount of dissolved O2? What happens to the amount of dissolved O2 when the pressure of O2 gas drops to 1.0 atm?

(a)

Interpretation Introduction

Interpretation The concentration of oxygen gas in the given condition has to be identified

Concept introduction:

Solubility of a gas: It is defined as the concentration of the dissolved gas in equilibrium with the substance in the gaseous state.

Henry’s law: The solubility of a gas in liquid is directly proportional to the gas pressure.

Sg= kHPg,where,Sgisthegassolubility(inmol/kg)kHis Henry's constant for gas in water at 25CPg is the partial pressure of the gaseous solute.

Explanation

Given:kH(O2 gas) = 1.3×10-3 mol/kg.barPO2=1.5 atm =1.5bar Concentration of  O2 gas (Sg)=  ? S

(b)

Interpretation Introduction

Interpretation The change in amount of dissolved oxygen has to be given if the pressure of oxygen in the flask is raised to 1.7atm and also if the pressure of oxygen gas drops to 1atm

Concept introduction:

Solubility of a gas: It is defined as the concentration of the dissolved gas in equilibrium with the substance in the gaseous state.

Henry’s law: The solubility of a gas in liquid is directly proportional to the gas pressure.

Sg= kHPg,where,Sgisthegassolubility(inmol/kg)kHis Henry's constant for gas in water at 25CPg is the partial pressure of the gaseous solute.

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Find more solutions based on key concepts 