The gas with highest partial pressure in the mixture of four gases; A (purple), B (black), C (green) and D 2 (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. Partial pressure = Mole fraction × P ( total ) Mole fraction is the ratio of moles of substance and total moles in the solution or mixture.

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Answer 1

Question

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.

Partial pressure = Mole fraction × P(total)

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.

Partial pressure = Mole fraction × P(total)

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.

Partial pressure = Mole fraction × P(total)

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

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Answer 2

Question

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.

Partial pressure = Mole fraction × P(total)

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.

Partial pressure = Mole fraction × P(total)

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.

Partial pressure = Mole fraction × P(total)

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

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 3

Question

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.

Partial pressure = Mole fraction × P(total)

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.

Partial pressure = Mole fraction × P(total)

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.

Partial pressure = Mole fraction × P(total)

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

Expert Solution & Answer

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Answer 4

Question

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.

Partial pressure = Mole fraction × P(total)

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.

Partial pressure = Mole fraction × P(total)

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.

Partial pressure = Mole fraction × P(total)

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

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 5

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.

Partial pressure = Mole fraction × P(total)

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.

Partial pressure = Mole fraction × P(total)

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.

Partial pressure = Mole fraction × P(total)

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

Answer 6

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.

Partial pressure = Mole fraction × P(total)

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

Answer 7

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.

Partial pressure = Mole fraction × P(total)

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

Answer 8

(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.

Partial pressure = Mole fraction × P(total)

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

Answer 9

(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.

Partial pressure = Mole fraction × P(total)

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

Answer 10

(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.

Partial pressure = Mole fraction × P(total)

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

Answer 11

(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.

Partial pressure = Mole fraction × P(total)

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

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 5 - Prob. 5.1P Ch. 5 - Prob. 5.2P Ch. 5 - Prob. 5.3P Ch. 5 - Prob. 5.4P Ch. 5 - Prob. 5.5P Ch. 5 - Prob. 5.6P Ch. 5 - Prob. 5.7P Ch. 5 - Prob. 5.8P Ch. 5 - The gravitational force exerted by Earth on an...Ch. 5 - Prob. 5.10P

Solution Summary: The author explains Dalton's law of partial pressure, which states that the total pressure of a gaseous mixture is equal to the sum of partially pressures of all gases.

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