∆H°r = B.E.(H-H)+B.E.(C=C) - 2×B.E.(C-H) -B.E.(C-C)
= 436 + 602 - 2×413 - 346 = -134 kJ
∆H°r = - 134 kJ (Answer)
Part A (in kilojoules) for the reaction of ethylene with hydrogen to yield ethane. Use the...
Ch
9 Q 39
Which is expected to have the largest carbom-oxygen bond
dissociation energy?
-HCOOH
-H2CO3
-CO2
-CO
9.106
Use the bond dissociation energies from the table provided to
calculate an approximate standard enthalpy in kilojoules for the
reaction of ethylene with hydrogen to yield ethane
Problem 9.106 Average Bond Dissociation Energies, D /mol) H-H 136 C-H410N - 390 0 F 1801-11 H-C 410 C-C 350 N-C 300 0-d 200 S-F 310 H-F 570 C-F 450 N-F 270 o-Br210...
The standard enthalpy change for the reaction of SO3 (g) with H2O(l) to yield H2SO4 (aq) is AH° = -227.8 kJ. Part A Use the following information S(s) + O2(g) +SO2(g), AH° = -296.8kJ SO2(g) + 1 O2(g) +S03 (g), AH° = -98.9kJ to calculate AH; for H2SO4(aq) (in kilojoules per mole). [For H2O(l), AH = -285.8kJ/mol]. Express your answer using four significant figures. O AXO A o ai ? AH; = Submit Request Answer Provide Feedback
H2C=CH2 + CI H2C=CH + HCI Use the table of bond dissociation energies above to calculate AH for this reaction, the first step in the free radical chlorination of ethene. Table of Bond Dissociation Enthalpies Bond BDE (kJ/mol) H2C=CH-H 464 H-I 297 H-Br 368 H-C1 431 H-F 568 ΔΗ: kJ/mol This reaction is:
Balance the equation for the complete combustion of ethane:
C2H6 (g) + O2 (g) ⟶⟶CO2
(g) + H2O (g). Calculate
ΔΔHofor the reaction per mole of
ethane using the given bond dissociation energies.
→CO2(g) + H2O (g). Calculate AH° for Balance the equation for the complete combustion of ethane: C2H6 (g) + O2(g) the reaction per mole of ethane using the given bond dissociation energies. Bond AH” (kJ/mol) C-C 347 H-O 467 C-H 413 O=0 498 C=0 799 CO 358
What is the theoretical yield of ethyl chloride in the reaction of 37.10 g of ethylene with 58.33 g of hydrogen chloride? (For ethylene, MW=28.0 amu; for hydrogen chloride, MW=36.5 amu; for ethyl chloride, MW=64.5 amu.) Report your answer to the nearest hundredth of a gram without units. H2C=CH2 + HCl → CH3CH2Cl
For the following reaction, 5.11 grams of ethylene (C2H4) are mixed with excess hydrogen gas. The reaction yields 4.67 grams of ethane (C2H6). hydrogen (g) - ethylene (C2HD (g)-ethane (C2H)(g) grams What is the theoretical yield of ethane (C2H6) ? What is the percent yield for this reaction ? %
12 e used to add hydrogen across dou 81. Hydrogenation reactions are used to add hydrogen ble bonds in hydrocarbons and other organic compounds 11 average bond energies to calculate AHrxn for the hydrogenation reaction. H2C=CH2(g) + H2(g) → H3C-CH3(g)
In the reaction of 43.43 g of ethylene with 45.7 g of hydrogen chloride, 65.1 g of ethyl chloride was isolated by an experimenter. What was the percent yield? (For ethylene, MW=28.0 amu; for hydrogen chloride, MW=36.5 amu; for ethyl chloride, MW=64.5 amu.) Report your answer to the tenths of a percent without units. H2C=CH2+ HCl → CH3CH2Cl
Compounds with carbon-carbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation C,H (9) + H2(g) + C H (9) Calculate the enthalpy change for this reaction, using the following combustion data: C4H4 () + 30 (g) + 2CO3(g) + 2H2O(); AH = -1411 kJ C, H(g) + O2(g) → 2002(g) + 3H2O(l); AH = -1560. kJ H2(g) + O2(g) H2O(l); AH = -286 kJ Enthalpy change - KJ Submit Answer Try Another Version 10 item...
Use average bond energies to calculate ΔHrxn for the following hydrogenation reaction: H2C=CH2(g)+H2(g)→H3C−CH3(g)