.The enthalpy change for the following reaction is -137 kJ. The enthalpy change for the following...
.The enthalpy change for the following reaction is -137 kJ. The enthalpy change for the following reaction is -137 kJ.
- C2H4(g) + H2(g) -> C2H6(g)
-
To analyze the reaction, first draw Lewis structures for all reactant and product molecules.
-
Estimate the C-C bond energy in C2H6(g) , using tabulated bond energies (linked above) for the remaining bonds
| H | C | N | O | F | Si | P | S | Cl | Br | I | |
|---|---|---|---|---|---|---|---|---|---|---|---|
|
H |
436 |
413 |
391 |
463 |
565 |
318 |
322 |
347 |
432 |
366 |
299 |
|
C |
413 |
346 |
305 |
358 |
485 |
--- |
--- |
272 |
339 |
285 |
213 |
|
N |
391 |
305 |
163 |
201 |
283 |
--- |
--- |
--- |
192 |
243 |
--- |
|
O |
463 |
358 |
201 |
146 |
184 |
452 |
335 |
--- |
218 |
201 |
201 |
|
F |
565 |
485 |
283 |
184 |
155 |
565 |
490 |
284 |
253 |
249 |
278 |
|
Si |
318 |
--- |
--- |
452 |
565 |
222 |
--- |
293 |
381 |
310 |
234 |
|
P |
322 |
--- |
--- |
335 |
490 |
--- |
201 |
--- |
326 |
--- |
184 |
|
S |
347 |
272 |
--- |
--- |
284 |
293 |
--- |
226 |
255 |
213 |
--- |
|
Cl |
432 |
339 |
192 |
218 |
253 |
381 |
326 |
255 |
242 |
216 |
208 |
|
Br |
366 |
285 |
243 |
201 |
249 |
310 |
--- |
213 |
216 |
193 |
175 |
|
I |
299 |
213 |
--- |
201 |
278 |
234 |
184 |
--- |
208 |
175 |
151 |
| Double Bonds (kJ/mol) |
Triple Bonds (kJ/mol) |
||
|---|---|---|---|
| C=C |
602 |
C≡C |
835 |
| O=O |
498 |
||
| C=O |
732 |
C≡O |
1072 |
| N=O |
607 |
||
| N=N |
418 |
N≡N |
945 |
| C=N |
615 |
C≡N |
887 |
Homework Answers
Add Answer to:
.The enthalpy change for the following reaction
is -137 kJ. The enthalpy change for the following...
The enthalpy change for the following reaction is 95.4 kJ. Using bond energies, estimate the N-H...
The enthalpy change for the following reaction is 95.4 kJ. Using bond energies, estimate the N-H bond energy in N2H4(g). N2(g) + 2H2(g) N2H4(g) kJ/mol The enthalpy change for the following reaction is -92.2 kJ. Using bond energies, estimate the H-H bond energy in H2(g). 2NH3(g) N2(g) + 3H2(g) kJ/mol D Single Bonds Multiple Bonds C N O F Si P S a Br 1 H 436 413 391 463 565 318 322 347 C 413 346 305 358 485...
Use average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction...
Use average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction CH4(g)2F2(g) CH2F2(g) + 2HF(g) To analyze the reaction, first draw Lewis structures for all reactant and product molecules Draw the reaction using separate sketchers for each species. Separate multiple reactants and/or products using the sign from the drop-down arrow. Separate reactants from products using the » symbol from the drop-down menu Remember to include nonbonding valence electrons in your Lewis structures. ChemDoodle HMolecularptructgre O...
a. b. For b is this table below: Bond Bond Energy, D (kJ/mol) C=0 1072 C1-C1...
a.
b. For b is this table below:
Bond Bond Energy, D (kJ/mol) C=0 1072 C1-C1 242 C-CI 339 C=0 732 Using the values of bond energy from the table above, estimate the enthalpy change for the following reaction: CO(g) + Cl2(9)—>COC12(E) DkJ Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: H2(g) + 12(8)—2HI(g) kJ Submit Answer Retry Entire Group 6 more group attempts remaining Single Bonds H C N O F Si P...
What is the enthalpy change for the reaction shown below? C2H2 + HCl -> CH2CHCl a. -34 kJ/mole...
What is the enthalpy change for the reaction shown below?
C2H2 + HCl -> CH2CHCl
a. -34 kJ/mole
b. -87 kJ/mole
c. +34 kJ/mole
d. +87 kJ/mole
Bond Dissociation Energies Average Single Bond Energies (kJ per mole) H 436414 389 464 569 293 318 339 431 368 297 347 293 351 439 289 264 259 330 276 238 159 201 272 201 243 138 184 368 351 201 159 540 490 285 255 197 176 213 226 360 289 Si...
Using the standard enthalpy of formation data, show how the standard enthalpy of formation of HF(g)...
Using the standard enthalpy of formation data, show how the standard enthalpy of formation of HF(g) can be used to determine the bond energy. (Enter unrounded values.) (a) bond energy calculated from standard enthalpy of formation kJ/mol (b) average bond enthalpy from the bond enthalpy table k]/mol Average Bond Enthalpies bondAH bond (kJ/mol) bond AHbond (kJ/mol) bond AH bond (kJ/mol) bond AH bond (kJ/mol) O-H 0-0 467 146 495 185 203 156 364 522 335 544 413 347 614 839...
Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ)...
Using the bond enthalpies in
the Average Bond Enthalpies table, determine the approximate
enthalpy (in kJ) for each of the following reactions. (Assume the
average bond enthalpy of the Cl–F bond is 254 kJ/mol.) (a) Cl2(g) +
3 F2(g) → 2 ClF3(g) (b) H2C=CH2(g) + H2(g) → H3CCH3(g) (c) 2
CH3(C=O)H(g) + 5 O2(g) → 4 CO2(g) + 4 H2O(g)
ITITIT Average Bond Enthalpies AH bond (kJ/mol) bond AHond (kJ/mol) bond AH bond (kJ/mol) bond bond AH bond (kJ/mol) С-Н...
Use the bond enthalpies in the table below to determine the enthalpy of reaction in the...
Use the bond enthalpies in the table below to determine the enthalpy of reaction in the following questions: Average Bond-Enthalpies- (kJ/mol) Single Bonds -H 41 3 348 293 358 485 N- 391 -H 463 -O 146 F-F 155 N-N 163 N-O 201 272 N-CI 200 N-Br 243 CI-P 253 N-I CI-CI 242 O-CI 203 -I 234 C-C Br-p 237 B-CI 218 Br-Br 193 339 327 S-Cl 253 S-Br 218 S-H 240 259 -X-H 436 567 431 366 299 208 175...
c.) Using the table and your complete Lewis structures of glucose, ethanol and carbon dioxide, calculate...
c.) Using the table and your complete Lewis structures of
glucose, ethanol and carbon dioxide, calculate the total energy in
kJ/mol required to break the bonds in one mole of each of the three
compounds. Show all calculations and appropriate units. Then
determine if the reaction is exothermic or endothermic.
reaction: C6H1206 -> 2 C2H5OH + 2 CO2
Table 4.4 Covalent Bond Energies (in kJ/mol) H C N O S F CI Br Single Bonds H 436 O ZOI 416...
Worksheet 8- Rev 10 Exercise B-Using Hess' Law to determine the enthalpy of a reaction. Using...
Worksheet 8- Rev 10 Exercise B-Using Hess' Law to determine the enthalpy of a reaction. Using the table below, calculate the enthalpy of each of the following reactions. For partial credit, show all of your work. Average Bond Energies (kj/mol) Multiple Bonds Single Bonds C C 614 149 H-H 432 391 160 272 1-1 N-H N-N 839 CC O-O 208 175 H-F H-CI 565 -CI 495 745 427 N-F 1-Br H-Br 363 C-O N-CI 200 H-I 1072 607 295 347...
Calculate the bond energy for the formation of boron trifluoride. Br-Br + 3 F- F -...
Calculate the bond energy for the formation of boron trifluoride. Br-Br + 3 F- F - 2 Br- F F-F 155 0-H 0-0 O-F 0-CI O-I 463 146 190 203 234 Cl-F 253 Cl-C1 242 Br-F 237 Br-Cl 218 Br-Br 193 Average Bond Enthalpies (kJ/mol) Single Bonds C-H 413 N-H 391 C-C 348 N-N 163 C-N 293 N-0 201 C-0 358 N-F 272 C-F 485 N-CI 200 C-C1328 N-Br 243 C-Br 276 C-1 240 H-H 436 C-S 259 H-F 567...
The enthalpy change for the following reaction is 95.4 kJ. Using bond energies, estimate the N-H bond energy in N2H4(g). N2(g) + 2H2(g) N2H4(g) kJ/mol The enthalpy change for the following reaction is -92.2 kJ. Using bond energies, estimate the H-H bond energy in H2(g). 2NH3(g) N2(g) + 3H2(g) kJ/mol D Single Bonds Multiple Bonds C N O F Si P S a Br 1 H 436 413 391 463 565 318 322 347 C 413 346 305 358 485...
Use average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction CH4(g)2F2(g) CH2F2(g) + 2HF(g) To analyze the reaction, first draw Lewis structures for all reactant and product molecules Draw the reaction using separate sketchers for each species. Separate multiple reactants and/or products using the sign from the drop-down arrow. Separate reactants from products using the » symbol from the drop-down menu Remember to include nonbonding valence electrons in your Lewis structures. ChemDoodle HMolecularptructgre O...
a.
b. For b is this table below:
Bond Bond Energy, D (kJ/mol) C=0 1072 C1-C1 242 C-CI 339 C=0 732 Using the values of bond energy from the table above, estimate the enthalpy change for the following reaction: CO(g) + Cl2(9)—>COC12(E) DkJ Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: H2(g) + 12(8)—2HI(g) kJ Submit Answer Retry Entire Group 6 more group attempts remaining Single Bonds H C N O F Si P...
What is the enthalpy change for the reaction shown below?
C2H2 + HCl -> CH2CHCl
a. -34 kJ/mole
b. -87 kJ/mole
c. +34 kJ/mole
d. +87 kJ/mole
Bond Dissociation Energies Average Single Bond Energies (kJ per mole) H 436414 389 464 569 293 318 339 431 368 297 347 293 351 439 289 264 259 330 276 238 159 201 272 201 243 138 184 368 351 201 159 540 490 285 255 197 176 213 226 360 289 Si...
Using the standard enthalpy of formation data, show how the standard enthalpy of formation of HF(g) can be used to determine the bond energy. (Enter unrounded values.) (a) bond energy calculated from standard enthalpy of formation kJ/mol (b) average bond enthalpy from the bond enthalpy table k]/mol Average Bond Enthalpies bondAH bond (kJ/mol) bond AHbond (kJ/mol) bond AH bond (kJ/mol) bond AH bond (kJ/mol) O-H 0-0 467 146 495 185 203 156 364 522 335 544 413 347 614 839...
Using the bond enthalpies in
the Average Bond Enthalpies table, determine the approximate
enthalpy (in kJ) for each of the following reactions. (Assume the
average bond enthalpy of the Cl–F bond is 254 kJ/mol.) (a) Cl2(g) +
3 F2(g) → 2 ClF3(g) (b) H2C=CH2(g) + H2(g) → H3CCH3(g) (c) 2
CH3(C=O)H(g) + 5 O2(g) → 4 CO2(g) + 4 H2O(g)
ITITIT Average Bond Enthalpies AH bond (kJ/mol) bond AHond (kJ/mol) bond AH bond (kJ/mol) bond bond AH bond (kJ/mol) С-Н...
Use the bond enthalpies in the table below to determine the enthalpy of reaction in the following questions: Average Bond-Enthalpies- (kJ/mol) Single Bonds -H 41 3 348 293 358 485 N- 391 -H 463 -O 146 F-F 155 N-N 163 N-O 201 272 N-CI 200 N-Br 243 CI-P 253 N-I CI-CI 242 O-CI 203 -I 234 C-C Br-p 237 B-CI 218 Br-Br 193 339 327 S-Cl 253 S-Br 218 S-H 240 259 -X-H 436 567 431 366 299 208 175...
c.) Using the table and your complete Lewis structures of
glucose, ethanol and carbon dioxide, calculate the total energy in
kJ/mol required to break the bonds in one mole of each of the three
compounds. Show all calculations and appropriate units. Then
determine if the reaction is exothermic or endothermic.
reaction: C6H1206 -> 2 C2H5OH + 2 CO2
Table 4.4 Covalent Bond Energies (in kJ/mol) H C N O S F CI Br Single Bonds H 436 O ZOI 416...
Worksheet 8- Rev 10 Exercise B-Using Hess' Law to determine the enthalpy of a reaction. Using the table below, calculate the enthalpy of each of the following reactions. For partial credit, show all of your work. Average Bond Energies (kj/mol) Multiple Bonds Single Bonds C C 614 149 H-H 432 391 160 272 1-1 N-H N-N 839 CC O-O 208 175 H-F H-CI 565 -CI 495 745 427 N-F 1-Br H-Br 363 C-O N-CI 200 H-I 1072 607 295 347...
Calculate the bond energy for the formation of boron trifluoride. Br-Br + 3 F- F - 2 Br- F F-F 155 0-H 0-0 O-F 0-CI O-I 463 146 190 203 234 Cl-F 253 Cl-C1 242 Br-F 237 Br-Cl 218 Br-Br 193 Average Bond Enthalpies (kJ/mol) Single Bonds C-H 413 N-H 391 C-C 348 N-N 163 C-N 293 N-0 201 C-0 358 N-F 272 C-F 485 N-CI 200 C-C1328 N-Br 243 C-Br 276 C-1 240 H-H 436 C-S 259 H-F 567...
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