Homework Answers
Bond energy, also known as bond enthalpy, is defined as the energy required for breaking the chemical bonds in a molecule. Bond energy is the measurement of the strength of a chemical bond. A chemical reaction involves the breaking and making of bonds. The amount of energy required for the breaking of bonds and the amount of energy released for bond-making is also represented as bond energy.
The arbitrary reaction is given below:
The formula to calculate the bond enthalpy or bond energy of reaction is given below:
The given data
Average 
bond energy in 
Number ofbond in 1 mol
The given reaction is
Average 
bond energy in 
Number of
bond in 1 mol
Average 
bond energy in 
Number of
bond in 1 mol
Number of
bond in 1 mol
Calculate the average bond energy of the reaction.
![Ан
reaction
bondenergy of reactant ->bondenergy of product
=2I(1xEv(CC)+(6xE(C- H)+(1xE (H-H)]-[8xE(C-H)]
avg
avg
avg
avg](http://img.homeworklib.com/questions/bca2b4c0-19b7-11ea-9d46-e9a2f3270b36.png?x-oss-process=image/resize,w_560)
Substitute the values.
![-65.07 [(1x347)+(6xE (CH)436)]-[8x415]
avg
(С-Н) - 2471.93
6xЕ
avg
C-H 411.98KJ /mol](http://img.homeworklib.com/questions/bd0061f0-19b7-11ea-affd-0f5f35d26ff0.png?x-oss-process=image/resize,w_560)
Therefore, the average bond energy of 
is
The given reaction is
Average bond energy in
Number ofbond in 2 mol
Average 
bond energy in 
Number of
bond in 1 mol
Number ofbond in 1 mol
Calculate the average bond energy of the reaction.
![bondenergy of reactant - >bond energy of product
AH
reaction
=I(1xE(C C)+(4xE(C-H)+(2x E
(H-H)]-[8xEav(C-H)]
avg
avg
avg](http://img.homeworklib.com/questions/c170c300-19b7-11ea-984b-f9ea9e8436bd.png?x-oss-process=image/resize,w_560)
Substitute the values.
![-202.21 [(x611)+(4xE(CH)(2x436)]-[8x415]
4xE (С-Н) 3 1634.79
C-H 408.70kJ/mol
avg
avg](http://img.homeworklib.com/questions/c1c9e010-19b7-11ea-9e17-057ce4ae5336.png?x-oss-process=image/resize,w_560)
Therefore, the average bond energy of 
is
The given reaction is
Average bond energy in
Number ofbond in 3 mol
Average 
bond energy in 
Number ofbond in 1 mol
Number ofbond in 1 mol
Calculate the average bond energy of the reaction.
![bondenergy of reactant - >bond energy of product
AH
reaction
=I(1xE(C C)+(2XEA(C-H)+(3xE (H-H)]-[8xEC-H)]
avg
avg
avg
avg](http://img.homeworklib.com/questions/c6216010-19b7-11ea-8cc3-a578b750056f.png?x-oss-process=image/resize,w_560)
Substitute the values.
![-376.74 [(x835)+(2x E(CH)+(3x436)]-[8x415]
|2xEv (CH) 800.26
avg
avg
C-H 400.13KJ /mol](http://img.homeworklib.com/questions/c65d1c80-19b7-11ea-b010-314238b049e5.png?x-oss-process=image/resize,w_560)
Therefore, the average bond energy of 
is
Add Answer to:
The average C - H bond energy in CH4 is 415 kJ / mol. Use the following data to calculate the average C - H bond energ...
For the reaction: H2(g)+C2H4(g)-->C2H6(g) Bond & Bond Enthalpy H-H 436.4 kJ/mole C-H 414 kJ/mol C-C 347...
For the reaction: H2(g)+C2H4(g)-->C2H6(g) Bond & Bond Enthalpy H-H 436.4 kJ/mole C-H 414 kJ/mol C-C 347 kJ/mol C=C 620 kJ/mol Substance & delta Hf H2 0 C2H4 52.3 C2H6 -84.7 (a) estimate the enthalpy of reaction, using the bond enthalpy values from the table in kJ/mol (b) Calculate the enthalpy of reaction, using standard enthalpies of formation
Calculate the average molar bond enthalpy of the carbon-hydrogen bond in a CH4 molecule. -- Given...
Calculate the average molar bond enthalpy of the carbon-hydrogen bond in a CH4 molecule. -- Given that (Delta)Hf [H(g)]= 218.0 kj/mol (Delta)Hf [C(g)]= 716.7 kJ/mol (Delta)Hf [CH4(g)]= -74.6 kJ/mol
Name: Quiz 9 CHE 1030 1. Using the following bond energies Bond Energy (kJ/mol) 839 413...
Name: Quiz 9 CHE 1030 1. Using the following bond energies Bond Energy (kJ/mol) 839 413 495 799 467 Bond C-H O-0 C-O O-H estimate the heat of combustion for 1 mol of acetylene: C2H2(g)+ O2(g) → 2CO2(g)+H2O(g) 2. Using the following data reactions: H2(g) + Cl2(g) → 2HCl(g) H2(g) → 2H(g) Cl2(g) 2CIg) AP (kJ) -184 432 239 calculate the energy of an H-Cl bond.
the bond energy for a c -h bond is about 413 kj/mol in ch4 but 380 kj/mol in chbr3. although these values are relatively...
the bond energy for a c -h bond is about 413 kj/mol in ch4 but 380 kj/mol in chbr3. although these values are relatively close in magnitude, they are different. explain why they are different on the basis of electronegativity.
The conversion of methane into products that contain two or more carbon atom, such as ethane,...
The conversion of methane into products that contain two or more
carbon atom, such as ethane, C2H2, is a very
important industrial chemical process. In principle, methane can be
converted directly into ethane and hydrogen.
(1) 2CH4(g) C2H6(g) +
H2(g)
In practice, however, this reaction is carried out in the
presence of oxygen:
(2) 2CH4(g) + 1/2 O2(g) C2H6(g) +
H2O(g)
a) Using the thermodynamic data at 298K, determine ΔG° for each
reaction.
ΔGf° (kJ/mol)
ΔGf° (kJ/mol)
CH4(g)
H2(g)
0...
Use deltaH and S to calculate DeltaG rxn... Use Delta H degree_f and S degree to...
Use deltaH and S to calculate DeltaG rxn...
Use Delta H degree_f and S degree to calculate Delta G degree rxn (Delta G degree sys) at 25 C for the reaction below: 4 KClO3 (s) rightarrow 3 KClO4 (s) + KCl (s) Delta H degree_f KClO3 = -397.7 kJ/mol; KClO4 = -432.8 kJ/mol; KCl = -436.7 kJ/mol S degree KClO3 = 143.1 kJ/mol; KClO4 = 151.0 kJ/mol; KCl = 82.6 kJ/mol
Part A. Find the average enthalpy of the PF bond in PF5(g) from the following standard...
Part A. Find the average enthalpy of the PF bond in PF5(g) from
the following standard molar enthalpies of formation (in kJ/mol):
PF5(g) (–1595), P(g) (315), F(g) (79).
Part B.
Using the bond energies from the table below estimate AH for the following reaction C2H2(g) + H2(g) → C2H4(g) Bond Bond energy [kJ/mol] [C-H 413 H-H 436 |C-C 348 C=C 614 csc 839
Use the table to answer questions about bond energies. Bond Bond Energy (KJ/mol) C—C 347 C=C...
Use the table to answer questions about bond energies. Bond Bond Energy (KJ/mol) C—C 347 C=C 611 C-H 414 C-O 360 C=O 736 O-O 142 O=O 498 H-O 464 (i) Calculate the bond energy for breaking all the bonds in a mole of methane, CH4 Express your answer numerically in kilojoules per mole. Change in Heat Ch4 ?=KJ/mol (ii) Calculate the bond energy for breaking all the bonds in a mole of O2 molecules? Express your answer numerically in kilojoules...
for the following rxn Use the standard enthalpies of formation to calculate AH° reaction. C2H4(g) +...
for the following rxn Use the standard enthalpies of formation to calculate AH° reaction. C2H4(g) + H2(g) + C2H6(g) ΔΗ° Substance (kJ/mol) C₂H4 52.4 C2H6 -84.68 0 -32.3 kJ -4.3 x 103 kJ 32.3 kJ 0 -137.1 kJ
Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: 2CO(g) +...
Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: 2CO(g) + 2NO(g)2CO2(g) + N2(g) kJ Bond Bond Energy (kJ/mol) C=C 602 H-H 436 C-H 413 C-C 346 Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: I2(g) + Cl2(g)2ICl(g) kJ Using the values of bond energy from the table above, estimate the enthalpy change for the following reaction: C2H4(g) + H2(g) C2H6(g) kJ
Name: Quiz 9 CHE 1030 1. Using the following bond energies Bond Energy (kJ/mol) 839 413 495 799 467 Bond C-H O-0 C-O O-H estimate the heat of combustion for 1 mol of acetylene: C2H2(g)+ O2(g) → 2CO2(g)+H2O(g) 2. Using the following data reactions: H2(g) + Cl2(g) → 2HCl(g) H2(g) → 2H(g) Cl2(g) 2CIg) AP (kJ) -184 432 239 calculate the energy of an H-Cl bond.
The conversion of methane into products that contain two or more
carbon atom, such as ethane, C2H2, is a very
important industrial chemical process. In principle, methane can be
converted directly into ethane and hydrogen.
(1) 2CH4(g) C2H6(g) +
H2(g)
In practice, however, this reaction is carried out in the
presence of oxygen:
(2) 2CH4(g) + 1/2 O2(g) C2H6(g) +
H2O(g)
a) Using the thermodynamic data at 298K, determine ΔG° for each
reaction.
ΔGf° (kJ/mol)
ΔGf° (kJ/mol)
CH4(g)
H2(g)
0...
Use deltaH and S to calculate DeltaG rxn...
Use Delta H degree_f and S degree to calculate Delta G degree rxn (Delta G degree sys) at 25 C for the reaction below: 4 KClO3 (s) rightarrow 3 KClO4 (s) + KCl (s) Delta H degree_f KClO3 = -397.7 kJ/mol; KClO4 = -432.8 kJ/mol; KCl = -436.7 kJ/mol S degree KClO3 = 143.1 kJ/mol; KClO4 = 151.0 kJ/mol; KCl = 82.6 kJ/mol
Part A. Find the average enthalpy of the PF bond in PF5(g) from
the following standard molar enthalpies of formation (in kJ/mol):
PF5(g) (–1595), P(g) (315), F(g) (79).
Part B.
Using the bond energies from the table below estimate AH for the following reaction C2H2(g) + H2(g) → C2H4(g) Bond Bond energy [kJ/mol] [C-H 413 H-H 436 |C-C 348 C=C 614 csc 839
for the following rxn Use the standard enthalpies of formation to calculate AH° reaction. C2H4(g) + H2(g) + C2H6(g) ΔΗ° Substance (kJ/mol) C₂H4 52.4 C2H6 -84.68 0 -32.3 kJ -4.3 x 103 kJ 32.3 kJ 0 -137.1 kJ
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