The partial pressure of ammonia in the container needs to be determined, when the reaction is complete at constant 1.00 atm and at constant volume. Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as: P × V = n × R × T Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation: ( P + n 2 a V 2 ) ( V- n b ) = nRT Hence P = nRT V-nb - n 2 a V 2

Question

Want to see more full solutions like this?

Answer 1

Question

Chapter 18, Problem 126CP

(a)

Interpretation Introduction

Interpretation: The partial pressure of ammonia in the container needs to be determined, when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(a)

Expert Solution

Answer to Problem 126CP

$Partial pressure of NH3= 0.5 atm$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

Calculate partial pressure of $NH3$ :

$Partial pressure of NH3=Ptotal× mole fractionPartial pressure of NH3= 1.0 atm × 0.5Partial pressure of NH3= 0.5 atm$

(b)

Interpretation Introduction

Interpretation: Interpret the mole fraction of ammonia in the container when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(b)

Expert Solution

Answer to Problem 126CP

$Mole fraction of NH3= 0.5$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

(c)

Interpretation Introduction

Interpretation:Interpret the volume of the container when the reaction complete if the initial pressure is 1.0 atm and volume is 15.0 L. The partial pressure of ammonia is 0.5 atm when reaction is complete.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(c)

Expert Solution

Answer to Problem 126CP

Volume = 10.0 L

Explanation of Solution

Initial volume is 15 L. Now, total initial moles are 2n. The final number of moles can be calculated by taking sum of moles of ammonia and moles of nitrogen.

$nf=2n3+2n3=4n3 mol$

At constant temperature, pressure can be calculated for an ideal gas as follows:

$Vini=Vfnf$

Putting the values,

$15 L2n=Vf 4n3Vf=10 L$

Thus, the final volume is 10 L.

Want to see more full solutions like this?

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

Students have asked these similar questions

The product on the right-hand side of this reaction can be prepared from two organic reactants, under the conditions shown above and below the arrow. Draw 1 and 2 below, in any arrangement you like. 1+2 NaBH₂CN H+ N Click and drag to start drawing a structure. X $

Explain what is the maximum absorbance of in which caffeine absorbs?

Explain reasons as to why the amount of caffeine extracted from both a singular extraction (5ml Mountain Dew) and a multiple extraction (2 x 5.0ml Mountain Dew) were severely high when compared to coca-cola?

Answer 2

Question

Chapter 18, Problem 126CP

(a)

Interpretation Introduction

Interpretation: The partial pressure of ammonia in the container needs to be determined, when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(a)

Expert Solution

Answer to Problem 126CP

$Partial pressure of NH3= 0.5 atm$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

Calculate partial pressure of $NH3$ :

$Partial pressure of NH3=Ptotal× mole fractionPartial pressure of NH3= 1.0 atm × 0.5Partial pressure of NH3= 0.5 atm$

(b)

Interpretation Introduction

Interpretation: Interpret the mole fraction of ammonia in the container when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(b)

Expert Solution

Answer to Problem 126CP

$Mole fraction of NH3= 0.5$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

(c)

Interpretation Introduction

Interpretation:Interpret the volume of the container when the reaction complete if the initial pressure is 1.0 atm and volume is 15.0 L. The partial pressure of ammonia is 0.5 atm when reaction is complete.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(c)

Expert Solution

Answer to Problem 126CP

Volume = 10.0 L

Explanation of Solution

Initial volume is 15 L. Now, total initial moles are 2n. The final number of moles can be calculated by taking sum of moles of ammonia and moles of nitrogen.

$nf=2n3+2n3=4n3 mol$

At constant temperature, pressure can be calculated for an ideal gas as follows:

$Vini=Vfnf$

Putting the values,

$15 L2n=Vf 4n3Vf=10 L$

Thus, the final volume is 10 L.

Want to see more full solutions like this?

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

Answer 3

Question

Chapter 18, Problem 126CP

(a)

Interpretation Introduction

Interpretation: The partial pressure of ammonia in the container needs to be determined, when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(a)

Expert Solution

Answer to Problem 126CP

$Partial pressure of NH3= 0.5 atm$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

Calculate partial pressure of $NH3$ :

$Partial pressure of NH3=Ptotal× mole fractionPartial pressure of NH3= 1.0 atm × 0.5Partial pressure of NH3= 0.5 atm$

(b)

Interpretation Introduction

Interpretation: Interpret the mole fraction of ammonia in the container when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(b)

Expert Solution

Answer to Problem 126CP

$Mole fraction of NH3= 0.5$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

(c)

Interpretation Introduction

Interpretation:Interpret the volume of the container when the reaction complete if the initial pressure is 1.0 atm and volume is 15.0 L. The partial pressure of ammonia is 0.5 atm when reaction is complete.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(c)

Expert Solution

Answer to Problem 126CP

Volume = 10.0 L

Explanation of Solution

Initial volume is 15 L. Now, total initial moles are 2n. The final number of moles can be calculated by taking sum of moles of ammonia and moles of nitrogen.

$nf=2n3+2n3=4n3 mol$

At constant temperature, pressure can be calculated for an ideal gas as follows:

$Vini=Vfnf$

Putting the values,

$15 L2n=Vf 4n3Vf=10 L$

Thus, the final volume is 10 L.

Want to see more full solutions like this?

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

Answer 4

Question

Chapter 18, Problem 126CP

(a)

Interpretation Introduction

Interpretation: The partial pressure of ammonia in the container needs to be determined, when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(a)

Expert Solution

Answer to Problem 126CP

$Partial pressure of NH3= 0.5 atm$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

Calculate partial pressure of $NH3$ :

$Partial pressure of NH3=Ptotal× mole fractionPartial pressure of NH3= 1.0 atm × 0.5Partial pressure of NH3= 0.5 atm$

(b)

Interpretation Introduction

Interpretation: Interpret the mole fraction of ammonia in the container when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(b)

Expert Solution

Answer to Problem 126CP

$Mole fraction of NH3= 0.5$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

(c)

Interpretation Introduction

Interpretation:Interpret the volume of the container when the reaction complete if the initial pressure is 1.0 atm and volume is 15.0 L. The partial pressure of ammonia is 0.5 atm when reaction is complete.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(c)

Expert Solution

Answer to Problem 126CP

Volume = 10.0 L

Explanation of Solution

Initial volume is 15 L. Now, total initial moles are 2n. The final number of moles can be calculated by taking sum of moles of ammonia and moles of nitrogen.

$nf=2n3+2n3=4n3 mol$

At constant temperature, pressure can be calculated for an ideal gas as follows:

$Vini=Vfnf$

Putting the values,

$15 L2n=Vf 4n3Vf=10 L$

Thus, the final volume is 10 L.

Want to see more full solutions like this?

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

Answer 5

Chapter 18, Problem 126CP

(a)

Interpretation Introduction

Interpretation: The partial pressure of ammonia in the container needs to be determined, when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(a)

Expert Solution

Answer to Problem 126CP

$Partial pressure of NH3= 0.5 atm$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

Calculate partial pressure of $NH3$ :

$Partial pressure of NH3=Ptotal× mole fractionPartial pressure of NH3= 1.0 atm × 0.5Partial pressure of NH3= 0.5 atm$

(b)

Interpretation Introduction

Interpretation: Interpret the mole fraction of ammonia in the container when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(b)

Expert Solution

Answer to Problem 126CP

$Mole fraction of NH3= 0.5$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

(c)

Interpretation Introduction

Interpretation:Interpret the volume of the container when the reaction complete if the initial pressure is 1.0 atm and volume is 15.0 L. The partial pressure of ammonia is 0.5 atm when reaction is complete.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(c)

Expert Solution

Answer to Problem 126CP

Volume = 10.0 L

Explanation of Solution

Initial volume is 15 L. Now, total initial moles are 2n. The final number of moles can be calculated by taking sum of moles of ammonia and moles of nitrogen.

$nf=2n3+2n3=4n3 mol$

At constant temperature, pressure can be calculated for an ideal gas as follows:

$Vini=Vfnf$

Putting the values,

$15 L2n=Vf 4n3Vf=10 L$

Thus, the final volume is 10 L.

Answer 6

Chapter 18, Problem 126CP

(a)

Interpretation Introduction

Interpretation: The partial pressure of ammonia in the container needs to be determined, when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(a)

Expert Solution

Answer to Problem 126CP

$Partial pressure of NH3= 0.5 atm$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

Calculate partial pressure of $NH3$ :

$Partial pressure of NH3=Ptotal× mole fractionPartial pressure of NH3= 1.0 atm × 0.5Partial pressure of NH3= 0.5 atm$

Answer 7

Chapter 18, Problem 126CP

(a)

Interpretation Introduction

Interpretation: The partial pressure of ammonia in the container needs to be determined, when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

Answer 8

(a)

Expert Solution

Answer to Problem 126CP

$Partial pressure of NH3= 0.5 atm$

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

Calculate partial pressure of $NH3$ :

$Partial pressure of NH3=Ptotal× mole fractionPartial pressure of NH3= 1.0 atm × 0.5Partial pressure of NH3= 0.5 atm$

Answer 13

(b)

Interpretation Introduction

Interpretation: Interpret the mole fraction of ammonia in the container when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(b)

Expert Solution

Answer to Problem 126CP

$Mole fraction of NH3= 0.5$

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

Answer 14

(b)

Interpretation Introduction

Interpretation: Interpret the mole fraction of ammonia in the container when the reaction is complete at constant 1.00 atm and at constant volume.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

Answer 15

(b)

Expert Solution

Answer to Problem 126CP

$Mole fraction of NH3= 0.5$

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

Number of $H2$ molecule = 6 molecules

Number of $N2$ gas = 6 molecules

The balance chemical equation for the formation of ammonia:

$N2+ 3 H2→2 NH3$

Hence 1 molecule of $N2$ reacts with 3 $H2$ molecule to form 2 molecule of $NH3$ .

Hence number of $N2$ reacts with 6 molecules of $H2$ :

$6 molecules of H2×1 molecules of N23 molecule of H2=2 molecules of N2$

Thus remaining $N2$ gas molecule = 6 − 2 = 4 molecules

Number of ammonia molecule formed = 2 x 2 = 4 molecules.

Total molecules at completion of reaction = 4 +4 = 16 molecules

Calculate mole fraction of ammonia:

$Mole fraction of NH3=4 molecule(4+4)molecules= 0.5$

Answer 20

(c)

Interpretation Introduction

Interpretation:Interpret the volume of the container when the reaction complete if the initial pressure is 1.0 atm and volume is 15.0 L. The partial pressure of ammonia is 0.5 atm when reaction is complete.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

(c)

Expert Solution

Answer to Problem 126CP

Volume = 10.0 L

Explanation of Solution

Initial volume is 15 L. Now, total initial moles are 2n. The final number of moles can be calculated by taking sum of moles of ammonia and moles of nitrogen.

$nf=2n3+2n3=4n3 mol$

At constant temperature, pressure can be calculated for an ideal gas as follows:

$Vini=Vfnf$

Putting the values,

$15 L2n=Vf 4n3Vf=10 L$

Thus, the final volume is 10 L.

Answer 21

(c)

Interpretation Introduction

Interpretation:Interpret the volume of the container when the reaction complete if the initial pressure is 1.0 atm and volume is 15.0 L. The partial pressure of ammonia is 0.5 atm when reaction is complete.

Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:

$P×V = n×R×T$

Usually gases do not follow ideal behavior under all conditions of pressure, temperature and volumes. The relation of P, V, n and T of real gases can be given by Vander Waals equation:

$(P + n2aV2) (V- n b) = nRT$

Hence $P = nRT V-nb - n2aV2$

Answer 22

(c)

Expert Solution

Answer to Problem 126CP

Volume = 10.0 L

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

Initial volume is 15 L. Now, total initial moles are 2n. The final number of moles can be calculated by taking sum of moles of ammonia and moles of nitrogen.

$nf=2n3+2n3=4n3 mol$