A gas sample has an initial pressure of 547 mmHg and an initial volume of 0 .500 L the pressure in atm should be determined when the volume of the sample is decreased by 225 mL assume constant temperature and constant number of moles of gas. Concept introduction: According to Boyle’s law, at constant temperature and constant number of moles of ideal gas the pressure of the gas is inversely proportional to its volume. P 1 V 1 = P 2 V 2 Where P is pressure and V is the volume of the gas in state 1 and 2 respectively. Correct answer: Correct answer is (d) option (a), (b) and (c) incorrect answer

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Answer 1

Question

Chapter 11, Problem 1SAQ

Interpretation Introduction

Interpretation: A gas sample has an initial pressure of $547 mmHg$ and an initial volume of $0.500 L$ the pressure in atm should be determined when the volume of the sample is decreased by $225 mL$ assume constant temperature and constant number of moles of gas.

Concept introduction: According to Boyle’s law, at constant temperature and constant number of moles of ideal gas the pressure of the gas is inversely proportional to its volume.

$P1V1 = P2V2$

Where P is pressure and V is the volume of the gas in state 1 and 2 respectively.

Correct answer:

Correct answer is (d) option (a), (b) and (c) incorrect answer

Expert Solution & Answer

Explanation of Solution

Reason for correct option: According to Boyle’s law

$P1V1 = P2V2$

Here the initial pressure $(P1) is 547mmHg,$ initial volume $(V1)is 0.500 L$ and final volume is $(V2) is 225 mL$ .

Converting 225 mL to L:

$V2=225 mL×1 L1000 mL(1 L = 1000 mL)= 0.225 L$

To calculate the final pressure $(P2)$ :

$P1V1 = P2V2P2=V1V2P1= 0.500 L0.225 L×547 mmHg=1215.5 mmHg×1 atm760 mmHg(1 atm=760mm Hg)=1.60 atm$

Thus the pressure will be $1.60 atm$ and the correct answer will be option (d).

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Answer 2

Question

Chapter 11, Problem 1SAQ

Interpretation Introduction

Interpretation: A gas sample has an initial pressure of $547 mmHg$ and an initial volume of $0.500 L$ the pressure in atm should be determined when the volume of the sample is decreased by $225 mL$ assume constant temperature and constant number of moles of gas.

Concept introduction: According to Boyle’s law, at constant temperature and constant number of moles of ideal gas the pressure of the gas is inversely proportional to its volume.

$P1V1 = P2V2$

Where P is pressure and V is the volume of the gas in state 1 and 2 respectively.

Correct answer:

Correct answer is (d) option (a), (b) and (c) incorrect answer

Expert Solution & Answer

Explanation of Solution

Reason for correct option: According to Boyle’s law

$P1V1 = P2V2$

Here the initial pressure $(P1) is 547mmHg,$ initial volume $(V1)is 0.500 L$ and final volume is $(V2) is 225 mL$ .

Converting 225 mL to L:

$V2=225 mL×1 L1000 mL(1 L = 1000 mL)= 0.225 L$

To calculate the final pressure $(P2)$ :

$P1V1 = P2V2P2=V1V2P1= 0.500 L0.225 L×547 mmHg=1215.5 mmHg×1 atm760 mmHg(1 atm=760mm Hg)=1.60 atm$

Thus the pressure will be $1.60 atm$ and the correct answer will be option (d).

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Answer 3

Question

Chapter 11, Problem 1SAQ

Interpretation Introduction

Interpretation: A gas sample has an initial pressure of $547 mmHg$ and an initial volume of $0.500 L$ the pressure in atm should be determined when the volume of the sample is decreased by $225 mL$ assume constant temperature and constant number of moles of gas.

Concept introduction: According to Boyle’s law, at constant temperature and constant number of moles of ideal gas the pressure of the gas is inversely proportional to its volume.

$P1V1 = P2V2$

Where P is pressure and V is the volume of the gas in state 1 and 2 respectively.

Correct answer:

Correct answer is (d) option (a), (b) and (c) incorrect answer

Expert Solution & Answer

Explanation of Solution

Reason for correct option: According to Boyle’s law

$P1V1 = P2V2$

Here the initial pressure $(P1) is 547mmHg,$ initial volume $(V1)is 0.500 L$ and final volume is $(V2) is 225 mL$ .

Converting 225 mL to L:

$V2=225 mL×1 L1000 mL(1 L = 1000 mL)= 0.225 L$

To calculate the final pressure $(P2)$ :

$P1V1 = P2V2P2=V1V2P1= 0.500 L0.225 L×547 mmHg=1215.5 mmHg×1 atm760 mmHg(1 atm=760mm Hg)=1.60 atm$

Thus the pressure will be $1.60 atm$ and the correct answer will be option (d).

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Answer 4

Question

Chapter 11, Problem 1SAQ

Interpretation Introduction

Interpretation: A gas sample has an initial pressure of $547 mmHg$ and an initial volume of $0.500 L$ the pressure in atm should be determined when the volume of the sample is decreased by $225 mL$ assume constant temperature and constant number of moles of gas.

Concept introduction: According to Boyle’s law, at constant temperature and constant number of moles of ideal gas the pressure of the gas is inversely proportional to its volume.

$P1V1 = P2V2$

Where P is pressure and V is the volume of the gas in state 1 and 2 respectively.

Correct answer:

Correct answer is (d) option (a), (b) and (c) incorrect answer

Expert Solution & Answer

Explanation of Solution

Reason for correct option: According to Boyle’s law

$P1V1 = P2V2$

Here the initial pressure $(P1) is 547mmHg,$ initial volume $(V1)is 0.500 L$ and final volume is $(V2) is 225 mL$ .

Converting 225 mL to L:

$V2=225 mL×1 L1000 mL(1 L = 1000 mL)= 0.225 L$

To calculate the final pressure $(P2)$ :

$P1V1 = P2V2P2=V1V2P1= 0.500 L0.225 L×547 mmHg=1215.5 mmHg×1 atm760 mmHg(1 atm=760mm Hg)=1.60 atm$

Thus the pressure will be $1.60 atm$ and the correct answer will be option (d).

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Answer 5

Chapter 11, Problem 1SAQ

Interpretation Introduction

Interpretation: A gas sample has an initial pressure of $547 mmHg$ and an initial volume of $0.500 L$ the pressure in atm should be determined when the volume of the sample is decreased by $225 mL$ assume constant temperature and constant number of moles of gas.

Concept introduction: According to Boyle’s law, at constant temperature and constant number of moles of ideal gas the pressure of the gas is inversely proportional to its volume.

$P1V1 = P2V2$

Where P is pressure and V is the volume of the gas in state 1 and 2 respectively.

Correct answer:

Correct answer is (d) option (a), (b) and (c) incorrect answer

Expert Solution & Answer

Explanation of Solution

Reason for correct option: According to Boyle’s law

$P1V1 = P2V2$

Here the initial pressure $(P1) is 547mmHg,$ initial volume $(V1)is 0.500 L$ and final volume is $(V2) is 225 mL$ .

Converting 225 mL to L:

$V2=225 mL×1 L1000 mL(1 L = 1000 mL)= 0.225 L$

To calculate the final pressure $(P2)$ :

$P1V1 = P2V2P2=V1V2P1= 0.500 L0.225 L×547 mmHg=1215.5 mmHg×1 atm760 mmHg(1 atm=760mm Hg)=1.60 atm$

Thus the pressure will be $1.60 atm$ and the correct answer will be option (d).

Answer 6

Chapter 11, Problem 1SAQ

Interpretation Introduction

Interpretation: A gas sample has an initial pressure of $547 mmHg$ and an initial volume of $0.500 L$ the pressure in atm should be determined when the volume of the sample is decreased by $225 mL$ assume constant temperature and constant number of moles of gas.

Concept introduction: According to Boyle’s law, at constant temperature and constant number of moles of ideal gas the pressure of the gas is inversely proportional to its volume.

$P1V1 = P2V2$

Where P is pressure and V is the volume of the gas in state 1 and 2 respectively.

Correct answer:

Correct answer is (d) option (a), (b) and (c) incorrect answer

Expert Solution & Answer

Explanation of Solution

Reason for correct option: According to Boyle’s law

$P1V1 = P2V2$

Here the initial pressure $(P1) is 547mmHg,$ initial volume $(V1)is 0.500 L$ and final volume is $(V2) is 225 mL$ .

Converting 225 mL to L:

$V2=225 mL×1 L1000 mL(1 L = 1000 mL)= 0.225 L$

To calculate the final pressure $(P2)$ :

$P1V1 = P2V2P2=V1V2P1= 0.500 L0.225 L×547 mmHg=1215.5 mmHg×1 atm760 mmHg(1 atm=760mm Hg)=1.60 atm$

Thus the pressure will be $1.60 atm$ and the correct answer will be option (d).

Answer 7

Chapter 11, Problem 1SAQ

Interpretation Introduction

Interpretation: A gas sample has an initial pressure of $547 mmHg$ and an initial volume of $0.500 L$ the pressure in atm should be determined when the volume of the sample is decreased by $225 mL$ assume constant temperature and constant number of moles of gas.

Concept introduction: According to Boyle’s law, at constant temperature and constant number of moles of ideal gas the pressure of the gas is inversely proportional to its volume.

$P1V1 = P2V2$

Where P is pressure and V is the volume of the gas in state 1 and 2 respectively.

Correct answer:

Correct answer is (d) option (a), (b) and (c) incorrect answer

Answer 8

Expert Solution & Answer

Explanation of Solution

Reason for correct option: According to Boyle’s law

$P1V1 = P2V2$

Here the initial pressure $(P1) is 547mmHg,$ initial volume $(V1)is 0.500 L$ and final volume is $(V2) is 225 mL$ .

Converting 225 mL to L:

$V2=225 mL×1 L1000 mL(1 L = 1000 mL)= 0.225 L$

To calculate the final pressure $(P2)$ :

$P1V1 = P2V2P2=V1V2P1= 0.500 L0.225 L×547 mmHg=1215.5 mmHg×1 atm760 mmHg(1 atm=760mm Hg)=1.60 atm$

Thus the pressure will be $1.60 atm$ and the correct answer will be option (d).

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

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