Solution Found!
(a) From the following data calculate the bond enthalpy
Chapter 9, Problem 110P(choose chapter or problem)
(a) From the following data calculate the bond enthalpy of the \(\mathrm{F}_{2}^{-}\) ion.
\(\mathrm{F}_2(g)\longrightarrow2\mathrm{F}(g)\quad\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \Delta H_{\mathrm{rxn}}^{\circ}=156.9\mathrm{\ kJ}/\mathrm{mol}\)
\(\mathrm{F}^-(g)\longrightarrow\mathrm{F}(g)+e^-\quad\ \ \ \ \ \ \ \ \ \Delta H_{\mathrm{rxn}}^{\circ}=333\mathrm{\ kJ}/\mathrm{mol}\)
\(\mathrm{F}_2^-(g)\longrightarrow\mathrm{F}_2(g)+e^-\ \ \ \ \ \ \ \quad\Delta H_{\mathrm{rxn}}^{\circ}=290\mathrm{\ kJ}/\mathrm{mol}\)
(b) Explain the difference between the bond enthalpies of \(\mathrm{F}_{2}\) and \(\mathrm{F}_{2}^{-}\).
Questions & Answers
QUESTION:
(a) From the following data calculate the bond enthalpy of the \(\mathrm{F}_{2}^{-}\) ion.
\(\mathrm{F}_2(g)\longrightarrow2\mathrm{F}(g)\quad\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \Delta H_{\mathrm{rxn}}^{\circ}=156.9\mathrm{\ kJ}/\mathrm{mol}\)
\(\mathrm{F}^-(g)\longrightarrow\mathrm{F}(g)+e^-\quad\ \ \ \ \ \ \ \ \ \Delta H_{\mathrm{rxn}}^{\circ}=333\mathrm{\ kJ}/\mathrm{mol}\)
\(\mathrm{F}_2^-(g)\longrightarrow\mathrm{F}_2(g)+e^-\ \ \ \ \ \ \ \quad\Delta H_{\mathrm{rxn}}^{\circ}=290\mathrm{\ kJ}/\mathrm{mol}\)
(b) Explain the difference between the bond enthalpies of \(\mathrm{F}_{2}\) and \(\mathrm{F}_{2}^{-}\).
ANSWER:Step 1 of 3
According to Hess law, the overall enthalpy change of a reaction is equal to the sum of the enthalpy changes involving in each and every individual steps in the reaction.
