Concept explainers
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Interpretation:
The
Concept introduction:
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(b)
Interpretation:
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Concept introduction:
The bond dissociation energy is denoted by
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Organic Chemistry
- 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 CCl4arrow_forward19 Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane using average bond enthalpies (use exam data sheet values). H–C≡C–H(g) + 2H2(g) → H3C–CH3(g)arrow_forwardUse the indicated average bond enthalpies to estimate the change in enthalpy, ΔHo, for the reaction between methane and iodine to produce iodomethane and hydrogen iodide: CH4(g) + I2(g) → CH3I(g) + HI(g) ΔHo = ? It may be helpful to draw the Lewis electron dot structure for each reactant and product; all reactants and products have single bonds. average bond enthalpies (kJ) C - H 413 , C - I 240 , H - I 299 , I - I 151 Express your answer in units of kilojoules, but do not include the units on your submitted answer.arrow_forward
- Calculate the enthalpy change (ΔH) for the reaction H2 + I2 → 2 HI,given the following bond dissociation energies: BE(H – H) = 436.4 kJ BE(I – I) = 151.0 kJ BE(H – I) = 298.3 kJarrow_forwardGiven the standard enthalpy changes for the following two reactions: (1) 2C(s) + H₂(g) → C₂H₂ (9) AH° = 226.7 kJ (2) 2C(s) + 2H₂(g) → C₂H₁ (9) ΔΗ° = 52.3 kJ What is the standard enthalpy change for the following reaction? (3) C₂H₂(g) + H2 (9) → C2H4 (9) AH° =? Standard enthalpy change = kJarrow_forwardFor 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-Narrow_forward
- Use the given bond dissociation energies to approximate the enthalpy change for the reaction of methane with molecular chlorine as shown in the reaction below. CH4(g) + 3Cl2₂(g) → CHCl3(g) + 3HCl(g) I BDE: C-H = 410 kJ/mol C-CI 330 kJ/mol a) -227 kJ b) -327 kJ c) -457 kJ d) +227 kJ e) + 327 kJ CI-CI = 243 kJ/mol H-CI = 432 kJ/mol H-H = 436 kJ/mol C-C= 350 kJ/molarrow_forwardCalculate the enthalpy change for the following reactions using the bond enthalpy given below. (Bond enthalpy/kJ : H−H = 436, C−H = 413, C=O = 799, O=O = 495, O−H = 463) (a) H2(g) + 1⁄2O2(g) → H2O(g) (b) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)arrow_forwardCalculate AH for the reaction NH3 (g) + CH4 (g) → HCN (g) + 3 H2 (g) , from the following data. N2 (g) + 3 H2 (g) → 2 NH3 (g) ΔΗ- – 91. 8 kJ /mol C (s, graphite) + 2 H2 (g) → CH4 (g) - 74. 9 kJ / mol AH = 2 C (s, graphite) + H2 (g) + N2 (g) → 2 HCN (g) AH = ΔΗ: 270. 3 kJ / molarrow_forward
- Which bond in each of the following pairs of bonds is the strongest?(a) C–C or C = C(b) C–N or C ≡ N(c) C ≡ O or C = O(d) H–F or H–Cl(e) C–H or O–H(f) C–N or C–Oarrow_forwardCovalent 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);arrow_forwardI 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: 467arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning