The given bonds ranked from strong to weak has to be explained. Concept introduction: Bond enthalpy: The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction. The enthalpy of reaction in gas phase is given by, ΔH o = ∑ BE(reaction) - ∑ BE(product)

Question

Want to see the full answer?

Answer 1

Question

Chapter 9, Problem 9.34QP

(a)

Interpretation Introduction

Interpretation:

The given bonds ranked from strong to weak has to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

(b)

Interpretation Introduction

Interpretation:

The enthalpy required to completely dissociate each of the product has to be compared.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

(c)

Interpretation Introduction

Interpretation:

The change of ΔH for each reaction of O-O instead O=O have to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Answer the following questions that relate to the chemistry of nitrogen. (a) Two nitrogen atoms combine to form a nitrogen molecule, as represented by the following equation. 2 N(g) ® N2(g) Using the table of average bond energies below, determine the enthalpy change, AH, for the reaction. Average Bond Energy (k) mol-1) Bond N-N 160 N=N 420 N°N 950 (b) The reaction between nitrogen and hydrogen to form ammonia is represented below. N2(g) + 3 H2(g)® 2 NH3(g) AH° = -92.2 kJ Predict the sign of the standard entropy change, AS', for the reaction. Justify your answer. (C) The value of AG° for the reaction represented in part (b) is negative at low temperatures but positive at high temperatures. Explain.

Hydrazine, N2H4, burns in oxygen as follows: N2H4 + O2 → N2 + 2H2O [The bond energies in kJ/mol are: N-H = 388; N-N 163; N≡N 944; O-H 463; O=O 496] Draw the chemical structures of the reactants and products and give the formula to calculate enthalpy change in a reaction, ΔH.

Use average bond enthalpy values to calculate ΔrH for the following reaction: 2NH3 + 3Cl2 → N2 + 6HCl

Answer 2

Question

Chapter 9, Problem 9.34QP

(a)

Interpretation Introduction

Interpretation:

The given bonds ranked from strong to weak has to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

(b)

Interpretation Introduction

Interpretation:

The enthalpy required to completely dissociate each of the product has to be compared.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

(c)

Interpretation Introduction

Interpretation:

The change of ΔH for each reaction of O-O instead O=O have to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 9, Problem 9.34QP

(a)

Interpretation Introduction

Interpretation:

The given bonds ranked from strong to weak has to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

(b)

Interpretation Introduction

Interpretation:

The enthalpy required to completely dissociate each of the product has to be compared.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

(c)

Interpretation Introduction

Interpretation:

The change of ΔH for each reaction of O-O instead O=O have to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 9, Problem 9.34QP

(a)

Interpretation Introduction

Interpretation:

The given bonds ranked from strong to weak has to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

(b)

Interpretation Introduction

Interpretation:

The enthalpy required to completely dissociate each of the product has to be compared.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

(c)

Interpretation Introduction

Interpretation:

The change of ΔH for each reaction of O-O instead O=O have to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 9, Problem 9.34QP

(a)

Interpretation Introduction

Interpretation:

The given bonds ranked from strong to weak has to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

(b)

Interpretation Introduction

Interpretation:

The enthalpy required to completely dissociate each of the product has to be compared.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

(c)

Interpretation Introduction

Interpretation:

The change of ΔH for each reaction of O-O instead O=O have to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Answer 6

Chapter 9, Problem 9.34QP

(a)

Interpretation Introduction

Interpretation:

The given bonds ranked from strong to weak has to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Answer 7

Chapter 9, Problem 9.34QP

(a)

Interpretation Introduction

Interpretation:

The given bonds ranked from strong to weak has to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Answer 8

(b)

Interpretation Introduction

Interpretation:

The enthalpy required to completely dissociate each of the product has to be compared.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Answer 9

(b)

Interpretation Introduction

Interpretation:

The enthalpy required to completely dissociate each of the product has to be compared.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Answer 10

(c)

Interpretation Introduction

Interpretation:

The change of ΔH for each reaction of O-O instead O=O have to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Answer 11

(c)

Interpretation Introduction

Interpretation:

The change of ΔH for each reaction of O-O instead O=O have to be explained.

Concept introduction:

Bond enthalpy:

The measure of stability of molecule is bond enthalpy. The change in enthalpy is related in breaking a specific bond of 1 mole of gaseous molecule. In solids and liquids bond enthalpies are affected by neighboring molecules. There is possibility to predict the enthalpy of reaction using the average bond enthalpies. Energy is always needed for the breaking of chemical bonds and release of energy always takes place with the formation of chemical bonds. The enthalpy of reaction is estimated by counting the total number of broken bonds and bonds formed in a reaction.

The enthalpy of reaction in gas phase is given by,

ΔHo= ∑BE(reaction) - ∑BE(product)

Answer 12

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 15

Ch. 9.1 - Represent the transfer of electrons from magnesium...Ch. 9.2 - Prob. 9.2E Ch. 9.2 - Prob. 9.3E Ch. 9.2 - Prob. 9.4E Ch. 9.2 - The following are electron configurations for some...Ch. 9.3 - Which has the larger radius, S or S2? Explain.Ch. 9.3 - Without looking at Table 9.3, arrange the...Ch. 9.3 - Prob. 9.7E Ch. 9.5 - Using electronegativities, decide which of the...Ch. 9.6 - Dichlorodifluoromethane, CCl2F2, is a gas used as...

Solution Summary: The author explains that the enthalpy of a reaction is equal to the sum of the bonds broken and the amount of energy released with the formation of chemical bonds.

Concept explainers

Videos

Want to see the full answer?

Chapter 9 Solutions