Question

Calculate the average bond energy of the sulfur-oxygen bonds in SO2 (in kJ/mol), given the following information. SF4(g) + 2 H2O(g) → SO2(g) + 4 HF(g) ΔH = -123 kJ Bond dissociation energies: S-F: 327 kJ/mol F-F: 154 kJ/mol H-F: 565 kJ/mol H-O: 467 kJ/mol

Name: calculate the average bond energy of the sulfur oxygen bonds in so2 in kjmol given the following information sf4g 2 h2og so2g 4 hfg h 123 kj bond dissociation energies sf 327 kjmol ff 154 kj 40484
Uploaded: 2023-06-14T14:40:13-08:00
Duration: 1 min 46 s
Channel: Adi S
Description: calculate the average bond energy of the sulfur oxygen bonds in so2 in kjmol given the following information sf4g 2 h2og so2g 4 hfg h 123 kj bond dissociation energies sf 327 kjmol ff 154 kj 40484

          Calculate the average bond energy of the sulfur-oxygen bonds in SO2 (in kJ/mol), given the following information.

SF4(g) + 2 H2O(g) → SO2(g) + 4 HF(g)

ΔH = -123 kJ

Bond dissociation energies:
S-F: 327 kJ/mol
F-F: 154 kJ/mol
H-F: 565 kJ/mol
H-O: 467 kJ/mol

Added by Alfredo F.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

06/14/2023

Step 1

First, we need to find the total energy of the bonds in the reactants and products. Reactants: 1 SF4 molecule has 4 S-F bonds: 4 * 327 kJ/mol = 1308 kJ/mol 2 H2O molecules have 4 O-H bonds: 4 * 467 kJ/mol = 1868 kJ/mol Total energy of reactants: 1308 + 1868 = Show more…

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Calculate the average bond energy of the sulfur-oxygen bonds in SO2 (in kJ/mol), given the following information. SF4(g) + 2 H2O(g) → SO2(g) + 4 HF(g) ΔH = -123 kJ Bond dissociation energies: S-F: 327 kJ/mol F-F: 154 kJ/mol H-F: 565 kJ/mol H-O: 467 kJ/mol