a. To determine: If the statement comparing the pressure of helium and neon is true or false.

Question

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Answer 1

Question

Chapter 11, Problem 11.79FU

Interpretation Introduction

a.

To determine: If the statement comparing the pressure of helium and neon is true or false.

Expert Solution

Explanation of Solution

As per the ideal gas equation:

$\begin{array}{l} PV = nRT -(1) \\ P = pressure ; V = volume \\ n = number of moles = \frac{m (mass)}{M (molar mass)} \\ R = Gas constant = 0 .0821 Latm/mol-K \\ T = Temperature \\ Equation (1) can be written as: \\ PV = \frac{m}{M} RT -(2) \end{array}$

According to equation (2), the pressure P of a gas is inversely proportional to its molar mass. The molar mass for $He = 4 g / mol$ and that of $Ne = 20 g / mol$ . Therefore, $He$ will have a higher pressure than $Ne$ . Hence, the given statement is true.

Interpretation Introduction

b.

To determine:

If the statement comparing the densities of helium and neon is true or false

Expert Solution

Explanation of Solution

We know that, the density is given as:

$Density (ρ) = \frac{mass (m)}{Volume (V)}$

Since, the mass and volume of both the gases are same. Therefore, ratio of mass and volume that is the density of both the gases are same.

Conclusion

Under the given conditions, $He$ will have a higher pressure than $Ne$ . However, the density of $Ne$ and $He$ are same.

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Answer 2

Question

Chapter 11, Problem 11.79FU

Interpretation Introduction

a.

To determine: If the statement comparing the pressure of helium and neon is true or false.

Expert Solution

Explanation of Solution

As per the ideal gas equation:

$\begin{array}{l} PV = nRT -(1) \\ P = pressure ; V = volume \\ n = number of moles = \frac{m (mass)}{M (molar mass)} \\ R = Gas constant = 0 .0821 Latm/mol-K \\ T = Temperature \\ Equation (1) can be written as: \\ PV = \frac{m}{M} RT -(2) \end{array}$

According to equation (2), the pressure P of a gas is inversely proportional to its molar mass. The molar mass for $He = 4 g / mol$ and that of $Ne = 20 g / mol$ . Therefore, $He$ will have a higher pressure than $Ne$ . Hence, the given statement is true.

Interpretation Introduction

b.

To determine:

If the statement comparing the densities of helium and neon is true or false

Expert Solution

Explanation of Solution

We know that, the density is given as:

$Density (ρ) = \frac{mass (m)}{Volume (V)}$

Since, the mass and volume of both the gases are same. Therefore, ratio of mass and volume that is the density of both the gases are same.

Conclusion

Under the given conditions, $He$ will have a higher pressure than $Ne$ . However, the density of $Ne$ and $He$ are same.

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Answer 3

Question

Chapter 11, Problem 11.79FU

Interpretation Introduction

a.

To determine: If the statement comparing the pressure of helium and neon is true or false.

Expert Solution

Explanation of Solution

As per the ideal gas equation:

$\begin{array}{l} PV = nRT -(1) \\ P = pressure ; V = volume \\ n = number of moles = \frac{m (mass)}{M (molar mass)} \\ R = Gas constant = 0 .0821 Latm/mol-K \\ T = Temperature \\ Equation (1) can be written as: \\ PV = \frac{m}{M} RT -(2) \end{array}$

According to equation (2), the pressure P of a gas is inversely proportional to its molar mass. The molar mass for $He = 4 g / mol$ and that of $Ne = 20 g / mol$ . Therefore, $He$ will have a higher pressure than $Ne$ . Hence, the given statement is true.

Interpretation Introduction

b.

To determine:

If the statement comparing the densities of helium and neon is true or false

Expert Solution

Explanation of Solution

We know that, the density is given as:

$Density (ρ) = \frac{mass (m)}{Volume (V)}$

Since, the mass and volume of both the gases are same. Therefore, ratio of mass and volume that is the density of both the gases are same.

Conclusion

Under the given conditions, $He$ will have a higher pressure than $Ne$ . However, the density of $Ne$ and $He$ are same.

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Answer 4

Question

Chapter 11, Problem 11.79FU

Interpretation Introduction

a.

To determine: If the statement comparing the pressure of helium and neon is true or false.

Expert Solution

Explanation of Solution

As per the ideal gas equation:

$\begin{array}{l} PV = nRT -(1) \\ P = pressure ; V = volume \\ n = number of moles = \frac{m (mass)}{M (molar mass)} \\ R = Gas constant = 0 .0821 Latm/mol-K \\ T = Temperature \\ Equation (1) can be written as: \\ PV = \frac{m}{M} RT -(2) \end{array}$

According to equation (2), the pressure P of a gas is inversely proportional to its molar mass. The molar mass for $He = 4 g / mol$ and that of $Ne = 20 g / mol$ . Therefore, $He$ will have a higher pressure than $Ne$ . Hence, the given statement is true.

Interpretation Introduction

b.

To determine:

If the statement comparing the densities of helium and neon is true or false

Expert Solution

Explanation of Solution

We know that, the density is given as:

$Density (ρ) = \frac{mass (m)}{Volume (V)}$

Since, the mass and volume of both the gases are same. Therefore, ratio of mass and volume that is the density of both the gases are same.

Conclusion

Under the given conditions, $He$ will have a higher pressure than $Ne$ . However, the density of $Ne$ and $He$ are same.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 11, Problem 11.79FU

Interpretation Introduction

a.

To determine: If the statement comparing the pressure of helium and neon is true or false.

Expert Solution

Explanation of Solution

As per the ideal gas equation:

$\begin{array}{l} PV = nRT -(1) \\ P = pressure ; V = volume \\ n = number of moles = \frac{m (mass)}{M (molar mass)} \\ R = Gas constant = 0 .0821 Latm/mol-K \\ T = Temperature \\ Equation (1) can be written as: \\ PV = \frac{m}{M} RT -(2) \end{array}$

According to equation (2), the pressure P of a gas is inversely proportional to its molar mass. The molar mass for $He = 4 g / mol$ and that of $Ne = 20 g / mol$ . Therefore, $He$ will have a higher pressure than $Ne$ . Hence, the given statement is true.

Interpretation Introduction

b.

To determine:

If the statement comparing the densities of helium and neon is true or false

Expert Solution

Explanation of Solution

We know that, the density is given as:

$Density (ρ) = \frac{mass (m)}{Volume (V)}$

Since, the mass and volume of both the gases are same. Therefore, ratio of mass and volume that is the density of both the gases are same.

Conclusion

Under the given conditions, $He$ will have a higher pressure than $Ne$ . However, the density of $Ne$ and $He$ are same.

Answer 6

Chapter 11, Problem 11.79FU

Interpretation Introduction

a.

To determine: If the statement comparing the pressure of helium and neon is true or false.

Expert Solution

Explanation of Solution

As per the ideal gas equation:

$\begin{array}{l} PV = nRT -(1) \\ P = pressure ; V = volume \\ n = number of moles = \frac{m (mass)}{M (molar mass)} \\ R = Gas constant = 0 .0821 Latm/mol-K \\ T = Temperature \\ Equation (1) can be written as: \\ PV = \frac{m}{M} RT -(2) \end{array}$

According to equation (2), the pressure P of a gas is inversely proportional to its molar mass. The molar mass for $He = 4 g / mol$ and that of $Ne = 20 g / mol$ . Therefore, $He$ will have a higher pressure than $Ne$ . Hence, the given statement is true.

Answer 7

Chapter 11, Problem 11.79FU

Interpretation Introduction

a.

To determine: If the statement comparing the pressure of helium and neon is true or false.

Answer 8

Expert Solution

Explanation of Solution

As per the ideal gas equation:

$\begin{array}{l} PV = nRT -(1) \\ P = pressure ; V = volume \\ n = number of moles = \frac{m (mass)}{M (molar mass)} \\ R = Gas constant = 0 .0821 Latm/mol-K \\ T = Temperature \\ Equation (1) can be written as: \\ PV = \frac{m}{M} RT -(2) \end{array}$

According to equation (2), the pressure P of a gas is inversely proportional to its molar mass. The molar mass for $He = 4 g / mol$ and that of $Ne = 20 g / mol$ . Therefore, $He$ will have a higher pressure than $Ne$ . Hence, the given statement is true.

Answer 9

Expert Solution

Answer 10

Expert Solution

Answer 11

Expert Solution

Answer 12

Interpretation Introduction

b.

To determine:

If the statement comparing the densities of helium and neon is true or false

Expert Solution

Explanation of Solution

We know that, the density is given as:

$Density (ρ) = \frac{mass (m)}{Volume (V)}$

Since, the mass and volume of both the gases are same. Therefore, ratio of mass and volume that is the density of both the gases are same.

Conclusion

Under the given conditions, $He$ will have a higher pressure than $Ne$ . However, the density of $Ne$ and $He$ are same.

Answer 13

Interpretation Introduction

b.

To determine:

If the statement comparing the densities of helium and neon is true or false

Answer 14

Expert Solution

Explanation of Solution

We know that, the density is given as:

$Density (ρ) = \frac{mass (m)}{Volume (V)}$

Since, the mass and volume of both the gases are same. Therefore, ratio of mass and volume that is the density of both the gases are same.

Answer 15

Expert Solution

Answer 16

Expert Solution

Answer 17

Expert Solution

Answer 18

Conclusion

Under the given conditions, $He$ will have a higher pressure than $Ne$ . However, the density of $Ne$ and $He$ are same.

Answer 19

Ch. 11.1 - Prob. 11.1QAP Ch. 11.1 - Prob. 11.2QAP Ch. 11.1 - Prob. 11.3QAP Ch. 11.1 - Prob. 11.4QAP Ch. 11.1 - Prob. 11.5QAP Ch. 11.1 - Prob. 11.6QAP Ch. 11.1 - Prob. 11.7QAP Ch. 11.1 - Prob. 11.8QAP Ch. 11.2 - Why do scuba divers need to exhale air when they...Ch. 11.2 - Why does a sealed bag of chips expand when you...

a. To determine: If the statement comparing the pressure of helium and neon is true or false.

Videos

a.

To determine: If the statement comparing the pressure of helium and neon is true or false.

Explanation of Solution

b.

To determine:

If the statement comparing the densities of helium and neon is true or false

Explanation of Solution

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Chapter 11 Solutions

a. To determine: If the statement comparing the pressure of helium and neon is true or false.

Videos

a. To determine: If the statement comparing the pressure of helium and neon is true or false.

Explanation of Solution

b. To determine: If the statement comparing the densities of helium and neon is true or false

Explanation of Solution

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Chapter 11 Solutions

a.

To determine: If the statement comparing the pressure of helium and neon is true or false.

b.

To determine:

If the statement comparing the densities of helium and neon is true or false