Multiple Choice
Using the bond energies provided, estimate the ΔH°rxn for the reaction: XeF2 + 2 F2 → XeF6.
11. Bonding & Molecular Structure
Bond Energy
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Consider the following equation:
Determine the bond enthalpy value for the F–S bond.
A
-2301.0 kJ/mol
B
335.5 kJ/mol
C
-1171.5 kJ/mol
D
1301.0 kJ/mol
Verified step by step guidance1
Identify the bonds broken and formed in the reaction. In the given reaction, the bonds broken are 2 S–H bonds and 3 F–F bonds. The bonds formed are 4 F–S bonds and 2 F–H bonds.
Use the bond energies provided to calculate the total energy required to break the bonds. The energy to break 2 S–H bonds is 2 * 347 kJ/mol, and the energy to break 3 F–F bonds is 3 * 159 kJ/mol.
Calculate the total energy released by forming the new bonds. The energy released by forming 4 F–S bonds is 4 * (unknown F–S bond energy), and the energy released by forming 2 F–H bonds is 2 * 565 kJ/mol.
Apply the formula for the enthalpy change of the reaction: ΔH = (Energy of bonds broken) - (Energy of bonds formed). Substitute the known values and the given ΔH of -1301 kJ/mol into the equation.
Solve the equation for the unknown F–S bond energy. Rearrange the equation to isolate the F–S bond energy and solve for its value.
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