SO2F2(g) has a ΔHºf = -858 kJ mol-1 and the S-F bond is 308.0 kJ mol-1
Determine the average S=O bond energy in SO2F2 in units of kJ.
To determine the average S=O bond energy in SO2F2, we first need to know the number of S=O bonds present in the molecule. By looking at the formula SO2F2, we can see that there are two oxygen atoms present. Therefore, there are two S=O bonds in the molecule.
Next, we need to calculate the total energy required to break all the S=O bonds in SO2F2. This can be calculated using the following equation:
Total Bond Energy = (Number of S=O bonds) x (S=O bond energy)
In this case, the S=O bond energy given is 308.0 kJ/mol. Therefore:
Total Bond Energy = (2 S=O bonds) x (308.0 kJ/mol) = 616.0 kJ/mol
So the total energy required to break all the S=O bonds in SO2F2 is 616.0 kJ/mol.
Finally, to determine the average S=O bond energy, we divide the total bond energy by the number of S=O bonds in the molecule:
Average S=O Bond Energy = (Total Bond Energy) / (Number of S=O bonds)
Average S=O Bond Energy = 616.0 kJ/mol / 2 S=O bonds = 308.0 kJ/mol
Therefore, the average S=O bond energy in SO2F2 is 308.0 kJ/mol.