We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
CH3CH3 . What is the value of AH in k mol-1 for the reaction CH2-CH2 +...
Using the table of average bond energies below, the AH for the reaction is k], C=0(g) + 2H2(g) → H3C-0-Hg) Bond: C-0 C=0 C=0 D(kJ/mol): 358 799 1072 C-H 413 H-H 436 O-H 463 -116 -276 +116 +276
Bond Dissociation Energies (for A-B Bond broken AH, kJ/mol Bond broken → A A4, kJ/mol + B) Bond broken mo H-H CH3CH2CH2-H (CH3)2CH-H (CH3)3C-H 436 423 413 400. H-Br 366 CH3CH2CH2-Br 294 (CH3)2CH-Br 298 (CH3)3C-Br292 Br-Br 193 H-CI 432 CH3CH2CH2-CI 354 (CH3)2CH-CI 355 (CH3)3C-CI 349 CI-CI 243 Alkane halogenation is a two-step reaction, as shown below. Using the table of bond dissociation energies, calculate the enthalpy of each step and the enthalpy of the overall reaction. Step 1: Number CH3CHCH3...
8. Ethanol is a common biofuel additive for gasoline. Estimate AH (kJ mol) for the combustion reaction of ethanol. Potentially useful bond energies are: H-H = 436 kJ/mol, O=0 = 499 kJ/mol, O-H 463 kl/mol, C=O = 799 kl/mol, C-O 358 kJ/mol, C-H= 411 kJ/mol, C-C = 346 kJ/mol a) -6000 b) - 1601 c) -1250 d) o e) + 4700
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
Using the bond energies from the table below estimate ∆H for the following reaction C2H2(g) + H2(g) → C2H4(g) C-H (413), H-H (436), C-C (348), C=C (614), C≡C (839) A) +165 kJ/mol B) -390. kJ/mol C) +390. kJ/mol D) –124 kJ/mol E) –165 kJ/mol
16) (10 pts.) Using the table of average bond energies below, what is AH for the reaction? HaC-O-H (g) → CEO(g) + 2H2(g) 413 Bond: Enthalpy (kJ/mol):358 1072 436 463 799
Question 1 The sign for AS in the following reaction is CH2=CH2(g) + H2(g) - CH3CH3(g) Which reaction is most likely to have a positive delta Ssys? CH3OH() - CH3OH(s) N2(g) + 3 H2(g) – 2 NH3(g) CH4(g) + H2O(g) - CO(g) + 3 H2(g) Na2CO3(s) + H2O(g) + CO2(g) - 2 NaHCO3(s)
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) ⇌ Si2H6(g) The conditions for this reaction are: PH2 = 1.83 bar PSi2H6 = 0.96 bar You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). ΔGf(Si2H6) = 127.3 kJ/mol ΔGf(H2) = 0 kJ/mol
Q-8(a). Use the bond energies provided to calculate AH; for the reaction below (3 marks) C2H419) + H29)C2H6(g) AHi ? Bond Energy (kJ mol-1) Bond 347 C-C C-H C=C 611 CEC 837 436 414 H-H
QUESTION 1 Calculate the heat of reaction (energy of reaction) in kJ/mol for the following reaction. Mind the correct sign of your answer value! 2 CO(g) + O2(g) →→2C02(g) Use the following bond energies for your calculation. Bond energies (kJ/mol) Bond Energy Bond Energy H-H 436 (-O 336 C-H 416 C=C 598 N–H 391 050 498 0-H 467 (=O 803 c-c 356 N=N 946 146 CEO 1073 LO