Part A Draw the kinetic product for the reaction Interactive 3D display mode CH, HCI Draw the molecule on the canvas by choosing buttons from the Tools (fo Template toolbars. The single bond is active by default. O ® H: 20 EXR CONT. Part C Draw the kinetic product for the reaction Interactive 3D display mode CH, HCI Draw the molecule on the canvas hy choosing b an Part B Draw the thermodynamic product for the reaction Interactive 3D display mode CH2 HCI

Part A Draw the kinetic product for the reaction Interactive 3D display mode CH, HCI Draw the molecule on the canvas by choosing buttons from the Tools (fo Template toolbars. The single bond is active by default. O ® H: 20 EXR CONT. Part C Draw the kinetic product for the reaction Interactive 3D display mode CH, HCI Draw the molecule on the canvas hy choosing b an Part B Draw the thermodynamic product for the reaction Interactive 3D display mode CH2 HCI

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter6: Alkanes & Alkenes

Section: Chapter Questions

Problem 19CTQ

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How do I (a) determine the energy change in the following reaction2 O2 + CH4→ CO2 + 2 H2Ogiven the following bond dissociation energies:C-C 340kJ/mol; C-H 420kJ/mol; O=O 490 kJ/mol; O-H 460 kJ/mol; C=O 720 kJ/mol. (b) Is the reaction exothermic or endothermic? Explaination?
Br2(at)+2NaI(aq) --> 2NaBr(aq)+I2(aq) Cl2(aq)+2NaBr(aq) --> NaCl(aq)+Br2 Which of the three halogens would you predict is the most stable, upon mixing with other halogens? Justify your answer.
32 Use the average bond energies to calculate the ∆H of the reaction: 4H--Cl + O2 → 2H—O—H + 2 Cl—Cl Data: ∆H (H-Cl) = 431 kj/mol ∆H (O-H) = 463 kj/mol ∆H (O2) = 494 kj/mol ∆H (Cl-Cl) = 243 kj/mol a. -130 b. -120 c. -150 d. -180
No plagiarism Please! Use the table to answer the question: Bond Bond Energy H-H 432 Cl-Cl 239 H-Cl 427 Explain how you would calculate the total change in bond energy for the reaction H2 + Cl2 -> 2HCl. How would you know if the reaction was endothermic or exothermic? State your answer in 3-5 sentences.
Consi‎der follo‎wing rea‎ction: HgO (s) -> Hg(l) + ½ O2 (g) Delta H = +90.7 kj/mol. Wh‎at qua‎ntity of h‎eat in kj/mol is req‎uired to prod‎uce on‎e m‎ole HgO? Wri‎te your answer wit‎hout units. Gi‎ven the fol‎lowing data 2Cl‎F(g) + O‎2(g) --> Cl2‎O(g) + F2‎O (g) De‎lta H= 167.4 kJ I 2Cl‎F3(g) + 2O‎2(g) --> Cl‎2O(g) + 3F2‎ O (g) Delta H= 341.4 kJ II 2 ‎F2(g) + O‎2(g) ---> 2F2O‎ (g) Delt‎a H= -43.4 kJ III Calc‎ulate the de‎lta H in kJ for below‎ reaction: ClF(g) + F2(g) ---> ClF3(g)
Which bond is most likely to be the location of a chemical reaction: C=N, C¬C, or C¬H?
Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following reaction: Use tabulated values of bond energies (Table 3-3) to estimate E for this reaction.
You will not find “hydroxide” in the stockroom, but you will find sodium hydroxide (NaOH) andpotassium hydroxide (KOH). Lithium hydroxide (LiOH) is expensive and used in spacecraft airfilters since hydroxide reacts with carbon dioxide, and lithium is lighter than sodium or potassium.Cesium and francium hydroxides are very expensive and little used. Is this information consistentwith your answer to the previous question?
Oxygen atoms can combine with ozone to form oxygen: O3(g) + O(g) 2 O2(g) rH = 392 kJ/mol-rxn Using rH and the bond dissociation enthalpy data in Table 8.8, estimate the bond dissociation enthalpy for the oxygen-oxygen bond in ozone, O3. How does your estimate compare with the energies of an OO single bond and an O=O double bond? Does the oxygen-oxygen bond dissociation enthalpy in ozone correlate with its bond order?
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What is the correct electron movement as reactant molecules interact for the incomplete reaction in the photo below?
Describe why this reaction is significant: H3AsO4 (aq) + 4Zn (s) + 8H+ (aq)-> AsH3 (g) + 4Zn 2+ (aq) + 4H2O (l)