The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below. C l 2 ( g ) ⇌ 2 C l ( g ) , K c = 1.7 × 10 − 5

Question

Want to see more full solutions like this?

Answer 1

Question

Chapter 5, Problem 5I.14E

(a)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

(a)

Expert Solution

Explanation of Solution

The required reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Cl]2[Cl2]

Given that, 5.0 mmol Cl2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Cl2(g) can be calculated as given below.

[Cl2]=molesvolume=5×10−3 mol2.00 L=0.0025M

An equilibrium table can be set up as given below.

Composition(M)Cl2ClInitial concentration0.00250Change in concentration−x+2xEquilibrium concentration0.0025−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(0.0025−x)

By assuming x≪0.0025, it can be written that 0.0025−x≃0.0025.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(0.0025−x)1.7×10−5=4x2(0.0025)x2=1.7×10−5×0.00254x=1.03×10-4[Cl2]=0.0025 M[Cl]=2x=2×1.03×10-4=2.06×10-4M

Therefore, the equilibrium concentrations of Cl2 and Cl in a reaction vessel are 0.0025M and 2.06×10-4 M respectively.

(b)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

(b)

Expert Solution

Explanation of Solution

The required reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Br]2[Br2]

Given that, 5.0 mol Br2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Br2(g) can be calculated as given below.

[Br2]=molesvolume=5 mol2.00 L=2.5M

An equilibrium table can be set up as given below.

Composition(M)Br2BrInitial concentration2.50Change in concentration−x+2xEquilibrium concentration2.5−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(2.5−x)

By assuming x≪2.5, it can be written that 2.5−x≃2.5.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(2.5−x)1.7×10−5=4x2(2.5)x2=1.7×10−5×2.54x=2.30×10-3[Br2]=2.5 M[Br]=2x=2×2.30×10-3=4.6×10-3M

Therefore, the equilibrium concentrations of Br2 and Br in a reaction vessel are 2.5M and 4.6×10-3 M respectively.

(c)

Interpretation Introduction

Interpretation:

The one which is thermodynamically more stable relative to its atoms at 1200 K has to be determined.

(c)

Expert Solution

Explanation of Solution

The percentage of dissociation of F2 and Br2 can be calculated as given below.

For Cl2:% of dissociation=dissociated amountoriginal amount×100% of dissociation=1.03×10−40.0025×100% of dissociation=4.12%For Br2:% of dissociation=2.30×10−32.5×100% of dissociation=0.092%

The percentage of dissociation of Br2 into its atoms is almost negligible than that of Cl2. Therefore, Br2 is thermodynamically more stable relative to its atoms at 1200 K.

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

Predict the major products of the following organic reaction: NC Δ ? Some important Notes: • Draw the major product, or products, of the reaction in the drawing area below. • If there aren't any products, because no reaction will take place, check the box below the drawing area instead. • Be sure to draw bonds carefully to show important geometric relationships between substituents. Note: if your answer contains a complicated ring structure, you must use one of the molecular fragment stamps (available in the menu at right) to enter the ring structure. You can add any substituents using the pencil tool in the usual way. Click and drag to start drawing a structure. Х а

Predict the major products of this organic reaction. Be sure you use dash and wedge bonds to show stereochemistry where it's important. + ☑ OH 1. TsCl, py .... 文 P 2. t-BuO K Click and drag to start drawing a structure.

Consider this organic reaction: ( Draw the major products of the reaction in the drawing area below. If there won't be any major products, because this reaction won't happen at a significant rate, check the box under the drawing area instead. Click and drag to start drawing a structure. Х : а ค 1

Answer 2

Question

Chapter 5, Problem 5I.14E

(a)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

(a)

Expert Solution

Explanation of Solution

The required reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Cl]2[Cl2]

Given that, 5.0 mmol Cl2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Cl2(g) can be calculated as given below.

[Cl2]=molesvolume=5×10−3 mol2.00 L=0.0025M

An equilibrium table can be set up as given below.

Composition(M)Cl2ClInitial concentration0.00250Change in concentration−x+2xEquilibrium concentration0.0025−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(0.0025−x)

By assuming x≪0.0025, it can be written that 0.0025−x≃0.0025.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(0.0025−x)1.7×10−5=4x2(0.0025)x2=1.7×10−5×0.00254x=1.03×10-4[Cl2]=0.0025 M[Cl]=2x=2×1.03×10-4=2.06×10-4M

Therefore, the equilibrium concentrations of Cl2 and Cl in a reaction vessel are 0.0025M and 2.06×10-4 M respectively.

(b)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

(b)

Expert Solution

Explanation of Solution

The required reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Br]2[Br2]

Given that, 5.0 mol Br2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Br2(g) can be calculated as given below.

[Br2]=molesvolume=5 mol2.00 L=2.5M

An equilibrium table can be set up as given below.

Composition(M)Br2BrInitial concentration2.50Change in concentration−x+2xEquilibrium concentration2.5−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(2.5−x)

By assuming x≪2.5, it can be written that 2.5−x≃2.5.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(2.5−x)1.7×10−5=4x2(2.5)x2=1.7×10−5×2.54x=2.30×10-3[Br2]=2.5 M[Br]=2x=2×2.30×10-3=4.6×10-3M

Therefore, the equilibrium concentrations of Br2 and Br in a reaction vessel are 2.5M and 4.6×10-3 M respectively.

(c)

Interpretation Introduction

Interpretation:

The one which is thermodynamically more stable relative to its atoms at 1200 K has to be determined.

(c)

Expert Solution

Explanation of Solution

The percentage of dissociation of F2 and Br2 can be calculated as given below.

For Cl2:% of dissociation=dissociated amountoriginal amount×100% of dissociation=1.03×10−40.0025×100% of dissociation=4.12%For Br2:% of dissociation=2.30×10−32.5×100% of dissociation=0.092%

The percentage of dissociation of Br2 into its atoms is almost negligible than that of Cl2. Therefore, Br2 is thermodynamically more stable relative to its atoms at 1200 K.

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 5, Problem 5I.14E

(a)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

(a)

Expert Solution

Explanation of Solution

The required reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Cl]2[Cl2]

Given that, 5.0 mmol Cl2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Cl2(g) can be calculated as given below.

[Cl2]=molesvolume=5×10−3 mol2.00 L=0.0025M

An equilibrium table can be set up as given below.

Composition(M)Cl2ClInitial concentration0.00250Change in concentration−x+2xEquilibrium concentration0.0025−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(0.0025−x)

By assuming x≪0.0025, it can be written that 0.0025−x≃0.0025.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(0.0025−x)1.7×10−5=4x2(0.0025)x2=1.7×10−5×0.00254x=1.03×10-4[Cl2]=0.0025 M[Cl]=2x=2×1.03×10-4=2.06×10-4M

Therefore, the equilibrium concentrations of Cl2 and Cl in a reaction vessel are 0.0025M and 2.06×10-4 M respectively.

(b)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

(b)

Expert Solution

Explanation of Solution

The required reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Br]2[Br2]

Given that, 5.0 mol Br2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Br2(g) can be calculated as given below.

[Br2]=molesvolume=5 mol2.00 L=2.5M

An equilibrium table can be set up as given below.

Composition(M)Br2BrInitial concentration2.50Change in concentration−x+2xEquilibrium concentration2.5−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(2.5−x)

By assuming x≪2.5, it can be written that 2.5−x≃2.5.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(2.5−x)1.7×10−5=4x2(2.5)x2=1.7×10−5×2.54x=2.30×10-3[Br2]=2.5 M[Br]=2x=2×2.30×10-3=4.6×10-3M

Therefore, the equilibrium concentrations of Br2 and Br in a reaction vessel are 2.5M and 4.6×10-3 M respectively.

(c)

Interpretation Introduction

Interpretation:

The one which is thermodynamically more stable relative to its atoms at 1200 K has to be determined.

(c)

Expert Solution

Explanation of Solution

The percentage of dissociation of F2 and Br2 can be calculated as given below.

For Cl2:% of dissociation=dissociated amountoriginal amount×100% of dissociation=1.03×10−40.0025×100% of dissociation=4.12%For Br2:% of dissociation=2.30×10−32.5×100% of dissociation=0.092%

The percentage of dissociation of Br2 into its atoms is almost negligible than that of Cl2. Therefore, Br2 is thermodynamically more stable relative to its atoms at 1200 K.

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 5, Problem 5I.14E

(a)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

(a)

Expert Solution

Explanation of Solution

The required reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Cl]2[Cl2]

Given that, 5.0 mmol Cl2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Cl2(g) can be calculated as given below.

[Cl2]=molesvolume=5×10−3 mol2.00 L=0.0025M

An equilibrium table can be set up as given below.

Composition(M)Cl2ClInitial concentration0.00250Change in concentration−x+2xEquilibrium concentration0.0025−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(0.0025−x)

By assuming x≪0.0025, it can be written that 0.0025−x≃0.0025.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(0.0025−x)1.7×10−5=4x2(0.0025)x2=1.7×10−5×0.00254x=1.03×10-4[Cl2]=0.0025 M[Cl]=2x=2×1.03×10-4=2.06×10-4M

Therefore, the equilibrium concentrations of Cl2 and Cl in a reaction vessel are 0.0025M and 2.06×10-4 M respectively.

(b)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

(b)

Expert Solution

Explanation of Solution

The required reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Br]2[Br2]

Given that, 5.0 mol Br2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Br2(g) can be calculated as given below.

[Br2]=molesvolume=5 mol2.00 L=2.5M

An equilibrium table can be set up as given below.

Composition(M)Br2BrInitial concentration2.50Change in concentration−x+2xEquilibrium concentration2.5−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(2.5−x)

By assuming x≪2.5, it can be written that 2.5−x≃2.5.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(2.5−x)1.7×10−5=4x2(2.5)x2=1.7×10−5×2.54x=2.30×10-3[Br2]=2.5 M[Br]=2x=2×2.30×10-3=4.6×10-3M

Therefore, the equilibrium concentrations of Br2 and Br in a reaction vessel are 2.5M and 4.6×10-3 M respectively.

(c)

Interpretation Introduction

Interpretation:

The one which is thermodynamically more stable relative to its atoms at 1200 K has to be determined.

(c)

Expert Solution

Explanation of Solution

The percentage of dissociation of F2 and Br2 can be calculated as given below.

For Cl2:% of dissociation=dissociated amountoriginal amount×100% of dissociation=1.03×10−40.0025×100% of dissociation=4.12%For Br2:% of dissociation=2.30×10−32.5×100% of dissociation=0.092%

The percentage of dissociation of Br2 into its atoms is almost negligible than that of Cl2. Therefore, Br2 is thermodynamically more stable relative to its atoms at 1200 K.

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 5, Problem 5I.14E

(a)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

(a)

Expert Solution

Explanation of Solution

The required reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Cl]2[Cl2]

Given that, 5.0 mmol Cl2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Cl2(g) can be calculated as given below.

[Cl2]=molesvolume=5×10−3 mol2.00 L=0.0025M

An equilibrium table can be set up as given below.

Composition(M)Cl2ClInitial concentration0.00250Change in concentration−x+2xEquilibrium concentration0.0025−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(0.0025−x)

By assuming x≪0.0025, it can be written that 0.0025−x≃0.0025.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(0.0025−x)1.7×10−5=4x2(0.0025)x2=1.7×10−5×0.00254x=1.03×10-4[Cl2]=0.0025 M[Cl]=2x=2×1.03×10-4=2.06×10-4M

Therefore, the equilibrium concentrations of Cl2 and Cl in a reaction vessel are 0.0025M and 2.06×10-4 M respectively.

(b)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

(b)

Expert Solution

Explanation of Solution

The required reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Br]2[Br2]

Given that, 5.0 mol Br2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Br2(g) can be calculated as given below.

[Br2]=molesvolume=5 mol2.00 L=2.5M

An equilibrium table can be set up as given below.

Composition(M)Br2BrInitial concentration2.50Change in concentration−x+2xEquilibrium concentration2.5−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(2.5−x)

By assuming x≪2.5, it can be written that 2.5−x≃2.5.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(2.5−x)1.7×10−5=4x2(2.5)x2=1.7×10−5×2.54x=2.30×10-3[Br2]=2.5 M[Br]=2x=2×2.30×10-3=4.6×10-3M

Therefore, the equilibrium concentrations of Br2 and Br in a reaction vessel are 2.5M and 4.6×10-3 M respectively.

(c)

Interpretation Introduction

Interpretation:

The one which is thermodynamically more stable relative to its atoms at 1200 K has to be determined.

(c)

Expert Solution

Explanation of Solution

The percentage of dissociation of F2 and Br2 can be calculated as given below.

For Cl2:% of dissociation=dissociated amountoriginal amount×100% of dissociation=1.03×10−40.0025×100% of dissociation=4.12%For Br2:% of dissociation=2.30×10−32.5×100% of dissociation=0.092%

The percentage of dissociation of Br2 into its atoms is almost negligible than that of Cl2. Therefore, Br2 is thermodynamically more stable relative to its atoms at 1200 K.

Answer 6

Chapter 5, Problem 5I.14E

(a)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

(a)

Expert Solution

Explanation of Solution

The required reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Cl]2[Cl2]

Given that, 5.0 mmol Cl2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Cl2(g) can be calculated as given below.

[Cl2]=molesvolume=5×10−3 mol2.00 L=0.0025M

An equilibrium table can be set up as given below.

Composition(M)Cl2ClInitial concentration0.00250Change in concentration−x+2xEquilibrium concentration0.0025−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(0.0025−x)

By assuming x≪0.0025, it can be written that 0.0025−x≃0.0025.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(0.0025−x)1.7×10−5=4x2(0.0025)x2=1.7×10−5×0.00254x=1.03×10-4[Cl2]=0.0025 M[Cl]=2x=2×1.03×10-4=2.06×10-4M

Therefore, the equilibrium concentrations of Cl2 and Cl in a reaction vessel are 0.0025M and 2.06×10-4 M respectively.

Answer 7

Chapter 5, Problem 5I.14E

(a)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

Answer 8

(a)

Expert Solution

Explanation of Solution

The required reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Cl]2[Cl2]

Given that, 5.0 mmol Cl2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Cl2(g) can be calculated as given below.

[Cl2]=molesvolume=5×10−3 mol2.00 L=0.0025M

An equilibrium table can be set up as given below.

Composition(M)Cl2ClInitial concentration0.00250Change in concentration−x+2xEquilibrium concentration0.0025−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(0.0025−x)

By assuming x≪0.0025, it can be written that 0.0025−x≃0.0025.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(0.0025−x)1.7×10−5=4x2(0.0025)x2=1.7×10−5×0.00254x=1.03×10-4[Cl2]=0.0025 M[Cl]=2x=2×1.03×10-4=2.06×10-4M

Therefore, the equilibrium concentrations of Cl2 and Cl in a reaction vessel are 0.0025M and 2.06×10-4 M respectively.

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

(b)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

(b)

Expert Solution

Explanation of Solution

The required reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Br]2[Br2]

Given that, 5.0 mol Br2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Br2(g) can be calculated as given below.

[Br2]=molesvolume=5 mol2.00 L=2.5M

An equilibrium table can be set up as given below.

Composition(M)Br2BrInitial concentration2.50Change in concentration−x+2xEquilibrium concentration2.5−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(2.5−x)

By assuming x≪2.5, it can be written that 2.5−x≃2.5.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(2.5−x)1.7×10−5=4x2(2.5)x2=1.7×10−5×2.54x=2.30×10-3[Br2]=2.5 M[Br]=2x=2×2.30×10-3=4.6×10-3M

Therefore, the equilibrium concentrations of Br2 and Br in a reaction vessel are 2.5M and 4.6×10-3 M respectively.

Answer 13

(b)

Interpretation Introduction

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

Answer 14

(b)

Expert Solution

Explanation of Solution

The required reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

The expression for equilibrium constant for the above reaction can be written as shown below,

Kc=[Br]2[Br2]

Given that, 5.0 mol Br2(g) was sealed into a reaction vessel of volume 2.0 L. The concentration of Br2(g) can be calculated as given below.

[Br2]=molesvolume=5 mol2.00 L=2.5M

An equilibrium table can be set up as given below.

Composition(M)Br2BrInitial concentration2.50Change in concentration−x+2xEquilibrium concentration2.5−x2x

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Kc=(2x)2(2.5−x)

By assuming x≪2.5, it can be written that 2.5−x≃2.5.

Now, the above equilibrium expression can be solved for x.

Kc=(2x)2(2.5−x)1.7×10−5=4x2(2.5)x2=1.7×10−5×2.54x=2.30×10-3[Br2]=2.5 M[Br]=2x=2×2.30×10-3=4.6×10-3M

Therefore, the equilibrium concentrations of Br2 and Br in a reaction vessel are 2.5M and 4.6×10-3 M respectively.

Answer 15

(b)

Expert Solution

Answer 16

(b)

Expert Solution

Answer 17

Expert Solution

Answer 18

(c)

Interpretation Introduction

Interpretation:

The one which is thermodynamically more stable relative to its atoms at 1200 K has to be determined.

(c)

Expert Solution

Explanation of Solution

The percentage of dissociation of F2 and Br2 can be calculated as given below.

For Cl2:% of dissociation=dissociated amountoriginal amount×100% of dissociation=1.03×10−40.0025×100% of dissociation=4.12%For Br2:% of dissociation=2.30×10−32.5×100% of dissociation=0.092%

The percentage of dissociation of Br2 into its atoms is almost negligible than that of Cl2. Therefore, Br2 is thermodynamically more stable relative to its atoms at 1200 K.

Answer 19

(c)

Interpretation Introduction

Interpretation:

The one which is thermodynamically more stable relative to its atoms at 1200 K has to be determined.

Answer 20

(c)

Expert Solution

Explanation of Solution

The percentage of dissociation of F2 and Br2 can be calculated as given below.

For Cl2:% of dissociation=dissociated amountoriginal amount×100% of dissociation=1.03×10−40.0025×100% of dissociation=4.12%For Br2:% of dissociation=2.30×10−32.5×100% of dissociation=0.092%

The percentage of dissociation of Br2 into its atoms is almost negligible than that of Cl2. Therefore, Br2 is thermodynamically more stable relative to its atoms at 1200 K.

Answer 21

(c)

Expert Solution

Answer 22

(c)

Expert Solution

Answer 23

Expert Solution

Answer 24

Ch. 5 - Prob. 5A.1AST Ch. 5 - Prob. 5A.1BST Ch. 5 - Prob. 5A.2AST Ch. 5 - Prob. 5A.2BST Ch. 5 - Prob. 5A.3AST Ch. 5 - Prob. 5A.3BST Ch. 5 - Prob. 5A.1E Ch. 5 - Prob. 5A.2E Ch. 5 - Prob. 5A.3E Ch. 5 - Prob. 5A.4E

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below. C l 2 ( g ) ⇌ 2 C l ( g ) , K c = 1.7 × 10 − 5

Interpretation: The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below. Cl2(g)⇌2Cl(g), Kc=1.7×10−5

Explanation of Solution

Interpretation: The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below. Br2(g)⇌2Br(g), Kc=1.7×10−5

Explanation of Solution

Interpretation: The one which is thermodynamically more stable relative to its atoms at 1200 K has to be determined.

Explanation of Solution

Want to see more full solutions like this?

Chapter 5 Solutions

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Cl2(g)⇌2Cl(g), Kc=1.7×10−5

Interpretation:

The equilibrium composition of the mixture in a reaction vessel of volume 2.00 L has to be calculated. The reaction is given below.

Br2(g)⇌2Br(g), Kc=1.7×10−5

Interpretation:

The one which is thermodynamically more stable relative to its atoms at 1200 K has to be determined.