AH° (kJ/mole) species H (g) O (g) H2O (g) H2O2 (g) 1. +218.0 (8H – ®YH¾ +249.1 -241.8 -136.4 Calculate the O-H bond energy in H2O. Use this to calculate the O-O bond energy in hydrogen peroxide, H-O-O-H. What is the bond energy in molecular oxygen? How does itcompare with that of H2O2? Comment.

AH° (kJ/mole) species H (g) O (g) H2O (g) H2O2 (g) 1. +218.0 (8H – ®YH¾ +249.1 -241.8 -136.4 Calculate the O-H bond energy in H2O. Use this to calculate the O-O bond energy in hydrogen peroxide, H-O-O-H. What is the bond energy in molecular oxygen? How does itcompare with that of H2O2? Comment.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 34QRT: Estimate ΔrH° for forming 2 mol ammonia from molecular nitrogen and molecular hydrogen. Is this...

See similar textbooks

Similar questions

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?
For each of the following covalent bonds: (a) use the symbols δ+ and δ- to indicate the direction of polarity (if any).(a) C-F; (b) N-Br; (c) B-C; (d) Si-H(b) Rank the following covalent bonds in order of increasing polarity. (i) C-H, O-H, N-H; (ii) C-N, C-O, B-O; (iii) C-P, C-S, C-N
I need this solution, Calculate the Enthalpy Change (ΔH) from average bond energies, which have been listed below in KJ/mol, for the following reaction and identify the nature of the reaction: CH3COOH + CH3OH → CH3COOCH3 + H2O [C‒H: 413; C‒C: 347; C=O: 745; C=C: 614; Cl‒Cl: 239, C‒O: 358; O‒H: 467
Which is the strongest bond energy? Cl(g) ΔH°f, = +121.3 kJ mol–1 CCl4(g) ΔH°f, = –95.98 kJ mol–1 HCl(g) ΔH°f, = –92.3 kJ mol–1 Question 8 options: Cl–Cl in Cl2 H–Cl in HCl C–Cl in CCl4
2-Butanol can be made by the reaction of 1-butene and water: H2 C=CH-CH,–CH3 (g) + H2O(g) → CH; CH(OH)CH2CH3 (g) a Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. Bond AH (kJ/mol) H-O 463 C=C 610 H-C 413 C-C 346 358 Enthalpy change = kJ b Calculate the enthalpy change for this reaction from enthalpies of formation. Substance AƒH (kJ/mol) CH3 CH(OH)CH2 CH3 (g) -293.1 H2O(g) -241.83 H2C=CH-CH2–CH3 (g) -0.1300 Enthalpy change = kJ
Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance A B C D H chemical symbol, chemical formula or Lewis structure H :0: 44 - C- C-H H - H 1 C I Ar H H | | - C - | 1 H H H Ag H CIO : 0: H boiling point ✓ (Choose one) 1 (highest) 2 3 4 (lowest) (Choose one) ✓ (Choose one) ✓
10. The following Lewis structures for (a) HCN, (b) C3H;, (c) SnOz, (d) BF3, (e)HOF are incorrect. Explain what is wrong with each one and give a correct structure for the molecule. (Relative positions of atoms are shown correctly.) (a) H-ëN (b) HCC-H (c) 0-Sn-0 (d) :F B :F: (e) H-O-F:
2RO; (aq) + 12 H* (aq) + 3 M (s) = RO (g)+3M²* (aq) + 6 H2O (1) = 3.86 V. R: 5 valence e-, electronegativity of R = 3.3 M: 2 valence e-, electronegativity of M = 0.5 O and H represent Oxygen and Hydrogen (the known elements, with their known properties) All atoms follow the octet rule; except for Hydrogen which follows the duet rule. b) Calculate the new cell potential if concentrations of all the reactants is deceased to 0.5 M, and the concentrations of all the products is increased to 0.5 M. Assume 6 mol electrons transferred in the reaction.
JA H;° of H2O(1) is -285.8 kJ/mol. calculate A H;° of MgO. The relevant reactions for these two heats of formation are: H2(g) + ½ O2(g) H20(1) and Mg(s) + ½ O2(g) - MgO(s) > -141.3 kj/mol a) -306.6 kj/mol b) -447.9 kj/mol c) d) -592.4 kj/mol 141.3 kj/mol f) Not even information given
For the following chemical reaction determine the heat of reaction (Bond enthalpy). Is this reaction exothermic or endothermic? H2C == CH2 + HCl ⟶⟶ CH3CH2Cl Bond Energy: C–H : 100 kcal/mol ; C=C: 145kcal/mol ; C-C: 83 kcal/mol ; H-Cl: 102 kcal/mol ; C-Cl : 81 kcal/mol bonds in reactant : 4 C-H , C=C, H-Cl bonds in Products: C-C, 5 C-H, C-Cl
Calculate AH for the reaction: 6 C(s) + 6 H2(g) + 3 O2(g) → C6H12O6(s) using the following three equations: C(s) + O2(g) → CO2(g) H2(g) + O2(g) → H₂O(1) C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(1) AH°=-285.8 kJ AH° = -285.8 kJ AH°=-2803.02 kJ
Covalent bonds: H―HC―HO―HO═O C≡O Bond energy (kJ/mol):4364154654981080Calculate the enthalpy change (H, in kJ/mol) for the following reaction and indicate whether the reaction is exothermic or endothermic.(*BE for C═Oin CO2)(a) CH4(g)+ H2O(g)CO(g)+ 3H2(g);