Chapter 5, Problem 5.29P

(a)

Interpretation Introduction

Interpretation: The gas with highest partial pressure in the mixture of four gases; A (purple), B (black), C (green) and D₂(orange) needs to be determined.

  

Concept Introduction:According to Dalton’s law of partial pressure, the total pressure of a gaseous mixture is equal to the sum of partial pressures of all gaseous components. Hence, the total pressure is larger than the partial pressure of both gaseous components.

  $\text{Partial pressure = Mole fraction }\times {\text{ P}}_{\left(\text{total}\right)}$

Mole fraction is the ratio of moles of substance and total moles in the solution or mixture.

(b)

Interpretation Introduction

Interpretation: The gas with the lowest partial pressure in the mixture of four gases; A (purple), B (black), C (green) and D₂(orange) needs to be determined.

  

Concept Introduction: According to Dalton’s law of partial pressure, the total pressure of a gaseous mixture is equal to the sum of partial pressures of all gaseous components. Hence the total pressure is larger than the partial pressure of both gaseous components.

  $\text{Partial pressure = Mole fraction }\times {\text{ P}}_{\left(\text{total}\right)}$

Mole fraction is the ratio of moles of substance and total moles in the solution or mixture.

(c)

Interpretation Introduction

Interpretation: The partial pressure of D₂ gas needs to be determined if the total pressure if the gas mixture is 0.75 atm in the mixture of four gases; A (purple), B (black), C (green) and D₂(orange).

  

Concept Introduction: According to Dalton’s law of partial pressure, the total pressure of a gaseous mixture is equal to the sum of partial pressures of all gaseous components. Hence, the total pressure is larger than the partial pressure of both gaseous components.

  $\text{Partial pressure = Mole fraction }\times {\text{ P}}_{\left(\text{total}\right)}$

Mole fraction is the ratio of moles of substance and total moles in the solution or mixture.