Pressure of gas in a full cylinder at 20 ° C when it empty cylinder weighs 0.74 kg has to be determined. Concept Introduction: An ideal gas contains a large number of randomly moving particles that are supposed to have perfectly elastic collisions among themselves. It is a theoretical concept. Gases that show perfect elastic collision are practically not possible. At higher T and lower P gases behave almost ideally. Ideal gas law is an equation of state for any hypothetical gas. Expression for ideal gas equation is as follows: P V = n R T Here, P is pressure of the gas. V is volume of gas. n denotes moles of gas. R is gas constant. T is temperature of gas.

Question

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Answer 1

Question

Chapter 3, Problem 3B.22E

(a)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it empty cylinder weighs 0.74 kg has to be determined.

Concept Introduction:

An ideal gas contains a large number of randomly moving particles that are supposed to have perfectly elastic collisions among themselves. It is a theoretical concept. Gases that show perfect elastic collision are practically not possible. At higher T and lower P gases behave almost ideally.

Ideal gas law is an equation of state for any hypothetical gas. Expression for ideal gas equation is as follows:

PV=nRT

Here,

P is pressure of the gas.

V is volume of gas.

n denotes moles of gas.

R is gas constant.

T is temperature of gas.

(a)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.74 kg)=0.3 kg(103 g1 kg)=300 g

Expression to calculate moles of CO2 is as follows:

(moles of CO2)=(mass of CO2molar mass of CO2) (1)

Substitute 300 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(300 g44.01 g/mol)=6.8166 mol

The conversion factor to convert 20 °C to Kelvin is as follows:

temperature in Kelvin=temperature in celsius+273.15=20 °C+273.15=293.15 K

Ideal gas equation is as follows:

PV=nRT (2)

Rearrange equation (2) to calculate P.

P=nRTV (3)

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 6.8166 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(6.8166 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=664.5868 bar

Hence, pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

(b)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g has to be determined.

Concept Introduction:

Refer to part (a)

(b)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g is 376.6010 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.87 kg)=0.17 kg(103 g1 kg)=170 g

Substitute 170 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(170 g44.01 g/mol)=3.8627 mol

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 3.8627 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(3.8627 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=376.6010 bar

Hence, pressure of gas in a full cylinder when it weighs 0.87 g is 376.6010 bar.

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Answer 2

Question

Chapter 3, Problem 3B.22E

(a)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it empty cylinder weighs 0.74 kg has to be determined.

Concept Introduction:

An ideal gas contains a large number of randomly moving particles that are supposed to have perfectly elastic collisions among themselves. It is a theoretical concept. Gases that show perfect elastic collision are practically not possible. At higher T and lower P gases behave almost ideally.

Ideal gas law is an equation of state for any hypothetical gas. Expression for ideal gas equation is as follows:

PV=nRT

Here,

P is pressure of the gas.

V is volume of gas.

n denotes moles of gas.

R is gas constant.

T is temperature of gas.

(a)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.74 kg)=0.3 kg(103 g1 kg)=300 g

Expression to calculate moles of CO2 is as follows:

(moles of CO2)=(mass of CO2molar mass of CO2) (1)

Substitute 300 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(300 g44.01 g/mol)=6.8166 mol

The conversion factor to convert 20 °C to Kelvin is as follows:

temperature in Kelvin=temperature in celsius+273.15=20 °C+273.15=293.15 K

Ideal gas equation is as follows:

PV=nRT (2)

Rearrange equation (2) to calculate P.

P=nRTV (3)

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 6.8166 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(6.8166 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=664.5868 bar

Hence, pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

(b)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g has to be determined.

Concept Introduction:

Refer to part (a)

(b)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g is 376.6010 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.87 kg)=0.17 kg(103 g1 kg)=170 g

Substitute 170 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(170 g44.01 g/mol)=3.8627 mol

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 3.8627 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(3.8627 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=376.6010 bar

Hence, pressure of gas in a full cylinder when it weighs 0.87 g is 376.6010 bar.

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Answer 3

Question

Chapter 3, Problem 3B.22E

(a)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it empty cylinder weighs 0.74 kg has to be determined.

Concept Introduction:

An ideal gas contains a large number of randomly moving particles that are supposed to have perfectly elastic collisions among themselves. It is a theoretical concept. Gases that show perfect elastic collision are practically not possible. At higher T and lower P gases behave almost ideally.

Ideal gas law is an equation of state for any hypothetical gas. Expression for ideal gas equation is as follows:

PV=nRT

Here,

P is pressure of the gas.

V is volume of gas.

n denotes moles of gas.

R is gas constant.

T is temperature of gas.

(a)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.74 kg)=0.3 kg(103 g1 kg)=300 g

Expression to calculate moles of CO2 is as follows:

(moles of CO2)=(mass of CO2molar mass of CO2) (1)

Substitute 300 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(300 g44.01 g/mol)=6.8166 mol

The conversion factor to convert 20 °C to Kelvin is as follows:

temperature in Kelvin=temperature in celsius+273.15=20 °C+273.15=293.15 K

Ideal gas equation is as follows:

PV=nRT (2)

Rearrange equation (2) to calculate P.

P=nRTV (3)

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 6.8166 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(6.8166 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=664.5868 bar

Hence, pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

(b)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g has to be determined.

Concept Introduction:

Refer to part (a)

(b)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g is 376.6010 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.87 kg)=0.17 kg(103 g1 kg)=170 g

Substitute 170 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(170 g44.01 g/mol)=3.8627 mol

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 3.8627 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(3.8627 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=376.6010 bar

Hence, pressure of gas in a full cylinder when it weighs 0.87 g is 376.6010 bar.

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Answer 4

Question

Chapter 3, Problem 3B.22E

(a)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it empty cylinder weighs 0.74 kg has to be determined.

Concept Introduction:

An ideal gas contains a large number of randomly moving particles that are supposed to have perfectly elastic collisions among themselves. It is a theoretical concept. Gases that show perfect elastic collision are practically not possible. At higher T and lower P gases behave almost ideally.

Ideal gas law is an equation of state for any hypothetical gas. Expression for ideal gas equation is as follows:

PV=nRT

Here,

P is pressure of the gas.

V is volume of gas.

n denotes moles of gas.

R is gas constant.

T is temperature of gas.

(a)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.74 kg)=0.3 kg(103 g1 kg)=300 g

Expression to calculate moles of CO2 is as follows:

(moles of CO2)=(mass of CO2molar mass of CO2) (1)

Substitute 300 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(300 g44.01 g/mol)=6.8166 mol

The conversion factor to convert 20 °C to Kelvin is as follows:

temperature in Kelvin=temperature in celsius+273.15=20 °C+273.15=293.15 K

Ideal gas equation is as follows:

PV=nRT (2)

Rearrange equation (2) to calculate P.

P=nRTV (3)

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 6.8166 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(6.8166 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=664.5868 bar

Hence, pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

(b)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g has to be determined.

Concept Introduction:

Refer to part (a)

(b)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g is 376.6010 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.87 kg)=0.17 kg(103 g1 kg)=170 g

Substitute 170 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(170 g44.01 g/mol)=3.8627 mol

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 3.8627 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(3.8627 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=376.6010 bar

Hence, pressure of gas in a full cylinder when it weighs 0.87 g is 376.6010 bar.

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Answer 5

Chapter 3, Problem 3B.22E

(a)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it empty cylinder weighs 0.74 kg has to be determined.

Concept Introduction:

An ideal gas contains a large number of randomly moving particles that are supposed to have perfectly elastic collisions among themselves. It is a theoretical concept. Gases that show perfect elastic collision are practically not possible. At higher T and lower P gases behave almost ideally.

Ideal gas law is an equation of state for any hypothetical gas. Expression for ideal gas equation is as follows:

PV=nRT

Here,

P is pressure of the gas.

V is volume of gas.

n denotes moles of gas.

R is gas constant.

T is temperature of gas.

(a)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.74 kg)=0.3 kg(103 g1 kg)=300 g

Expression to calculate moles of CO2 is as follows:

(moles of CO2)=(mass of CO2molar mass of CO2) (1)

Substitute 300 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(300 g44.01 g/mol)=6.8166 mol

The conversion factor to convert 20 °C to Kelvin is as follows:

temperature in Kelvin=temperature in celsius+273.15=20 °C+273.15=293.15 K

Ideal gas equation is as follows:

PV=nRT (2)

Rearrange equation (2) to calculate P.

P=nRTV (3)

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 6.8166 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(6.8166 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=664.5868 bar

Hence, pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

(b)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g has to be determined.

Concept Introduction:

Refer to part (a)

(b)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g is 376.6010 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.87 kg)=0.17 kg(103 g1 kg)=170 g

Substitute 170 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(170 g44.01 g/mol)=3.8627 mol

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 3.8627 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(3.8627 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=376.6010 bar

Hence, pressure of gas in a full cylinder when it weighs 0.87 g is 376.6010 bar.

Answer 6

Chapter 3, Problem 3B.22E

(a)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it empty cylinder weighs 0.74 kg has to be determined.

Concept Introduction:

An ideal gas contains a large number of randomly moving particles that are supposed to have perfectly elastic collisions among themselves. It is a theoretical concept. Gases that show perfect elastic collision are practically not possible. At higher T and lower P gases behave almost ideally.

Ideal gas law is an equation of state for any hypothetical gas. Expression for ideal gas equation is as follows:

PV=nRT

Here,

P is pressure of the gas.

V is volume of gas.

n denotes moles of gas.

R is gas constant.

T is temperature of gas.

(a)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.74 kg)=0.3 kg(103 g1 kg)=300 g

Expression to calculate moles of CO2 is as follows:

(moles of CO2)=(mass of CO2molar mass of CO2) (1)

Substitute 300 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(300 g44.01 g/mol)=6.8166 mol

The conversion factor to convert 20 °C to Kelvin is as follows:

temperature in Kelvin=temperature in celsius+273.15=20 °C+273.15=293.15 K

Ideal gas equation is as follows:

PV=nRT (2)

Rearrange equation (2) to calculate P.

P=nRTV (3)

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 6.8166 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(6.8166 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=664.5868 bar

Hence, pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

Answer 7

Chapter 3, Problem 3B.22E

(a)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it empty cylinder weighs 0.74 kg has to be determined.

Concept Introduction:

An ideal gas contains a large number of randomly moving particles that are supposed to have perfectly elastic collisions among themselves. It is a theoretical concept. Gases that show perfect elastic collision are practically not possible. At higher T and lower P gases behave almost ideally.

Ideal gas law is an equation of state for any hypothetical gas. Expression for ideal gas equation is as follows:

PV=nRT

Here,

P is pressure of the gas.

V is volume of gas.

n denotes moles of gas.

R is gas constant.

T is temperature of gas.

Answer 8

(a)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.74 kg)=0.3 kg(103 g1 kg)=300 g

Expression to calculate moles of CO2 is as follows:

(moles of CO2)=(mass of CO2molar mass of CO2) (1)

Substitute 300 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(300 g44.01 g/mol)=6.8166 mol

The conversion factor to convert 20 °C to Kelvin is as follows:

temperature in Kelvin=temperature in celsius+273.15=20 °C+273.15=293.15 K

Ideal gas equation is as follows:

PV=nRT (2)

Rearrange equation (2) to calculate P.

P=nRTV (3)

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 6.8166 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(6.8166 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=664.5868 bar

Hence, pressure of gas in a full cylinder at 20 °C is 664.5868 bar.

Answer 13

(b)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g has to be determined.

Concept Introduction:

Refer to part (a)

(b)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g is 376.6010 bar.

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.87 kg)=0.17 kg(103 g1 kg)=170 g

Substitute 170 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(170 g44.01 g/mol)=3.8627 mol

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 3.8627 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(3.8627 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=376.6010 bar

Hence, pressure of gas in a full cylinder when it weighs 0.87 g is 376.6010 bar.

Answer 14

(b)

Interpretation Introduction

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g has to be determined.

Concept Introduction:

Refer to part (a)

Answer 15

(b)

Expert Solution

Answer to Problem 3B.22E

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g is 376.6010 bar.

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

Mass of CO2 in cylinder is calculated as follows:

weight of CO2=(weight of full cylinder)−(weight of empty cylinder)=(1.04 kg)−(0.87 kg)=0.17 kg(103 g1 kg)=170 g

Substitute 170 g for mass of CO2 and 44.01 g/mol for molar mass of CO2 in equation (1) to calculate moles of CO2.

(moles of CO2)=(170 g44.01 g/mol)=3.8627 mol

Substitute 250 mL for V, 8.31446×10−2 L⋅bar⋅K−1⋅mol−1 for R, 3.8627 mol for n and 293.15 K for T in equation (3) to calculate P.

P=(3.8627 mol)(8.31446×10−2 L⋅bar⋅K−1⋅mol−1 )(293.15 K)(250 mL)(0.001 L1 mL)=376.6010 bar

Hence, pressure of gas in a full cylinder when it weighs 0.87 g is 376.6010 bar.

Answer 20

Ch. 3 - Prob. 3A.1AST Ch. 3 - Prob. 3A.1BST Ch. 3 - Prob. 3A.2AST Ch. 3 - Prob. 3A.2BST Ch. 3 - Prob. 3A.3AST Ch. 3 - Prob. 3A.3BST Ch. 3 - Prob. 3A.1E Ch. 3 - Prob. 3A.2E Ch. 3 - Prob. 3A.3E Ch. 3 - Prob. 3A.4E

Videos

Answer to Problem 3B.22E

Explanation of Solution

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g has to be determined.

Concept Introduction:

Refer to part (a)

Answer to Problem 3B.22E

Explanation of Solution

Want to see more full solutions like this?

Chapter 3 Solutions

Videos

Answer to Problem 3B.22E

Explanation of Solution

Interpretation: Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g has to be determined. Concept Introduction: Refer to part (a)

Answer to Problem 3B.22E

Explanation of Solution

Want to see more full solutions like this?

Chapter 3 Solutions

Interpretation:

Pressure of gas in a full cylinder at 20 °C when it weighs 0.87 g has to be determined.

Concept Introduction:

Refer to part (a)