Question

Using the standard enthalpy of formation data in Appendix G, determine which bond is stronger: the P–Cl bond in PCl₃(g) or in PCl₅(g)?

Answer 1

To determine which P-Cl bond is stronger in PCl3(g) or PCl5(g), we compare their standard enthalpies of formation; the compound with the more negative value has the stronger P-Cl bond.

Step-by-step explanation:

To determine which P-Cl bond is stronger, we need to compare the standard enthalpies of formation (∆H°f) for PCl₃(g) and PCl₅3(g). The bond strength can generally be approximated by analyzing how much energy is required to form the compounds. A more negative enthalpy of formation indicates that more energy is released when the compound forms, suggesting stronger bonds within the compound. Without the specific enthalpy values provided in Appendix G, we can't perform the exact calculation here. However, we can say that the compound with the more negative ∆H°f will have the stronger P-Cl bond. Remember, to apply these principles, you'd look up the standard enthalpies of formation in Appendix G for both PCl₃(g) and PCl₅3(g), and compare them directly. The value that is more negative will indicate the stronger bond.