Use Table 8.4 to estimate the enthalpy change for each of the following reactions: (a) \(\mathrm{H}_{2} \mathrm{C}=\mathrm{O}(g)+\mathrm{HCl}(g) \longrightarrow \mathrm{H}_{3} \mathrm{C}-\mathrm{O}-\mathrm{Cl}(g)\) (b) \(\mathrm{H}_{2} \mathrm{O}_{2}(g)+2 \mathrm{CO}(g) \longrightarrow \mathrm{H}_{2}(g)+2 \mathrm{CO}_{2}(g)\) (c) \(3 \mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}(g) \longrightarrow \mathrm{C}_{6} \mathrm{H}_{12}(g)\) (the six carbon atoms form a six-membered ring with two \(\mathrm{H}\) atoms on each \(\mathrm{C}\) atom \()\)

Look at each chemical reaction and identify the initial bonds that are broken in the reactants and the new bonds that are formed in the products. (a) $\mathrm{H}_{2} \mathrm{C}=\mathrm{O}(g)+\mathrm{HCl}(g) \longrightarrow \mathrm{H}_{3} \mathrm{C}-\mathrm{O}-\mathrm{Cl}(g)$ Bonds broken: H-C, C=O, and H-Cl Bonds formed: H-C, C-O, and O-Cl (b) $\mathrm{H}_{2} \mathrm{O}_{2}(g)+2 \mathrm{CO}(g) \longrightarrow \mathrm{H}_{2}(g)+2 \mathrm{CO}_{2}(g)$ Bonds broken: H-O, O-O, 2 C≡O Bonds formed: H-H, and 4 C=O (c) $3 \mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}(g) \longrightarrow \mathrm{C}_{6} \mathrm{H}_{12}(g)$ (the six carbon atoms form a six-membered ring with two \(\mathrm{H}\) atoms on each \(\mathrm{C}\) atom \()\) Bonds broken: 6 H-C, 3 C=C Bonds formed: 12 H-C, 6 C-C

Consult Table 8.4 to find the bond enthalpies for each bond broken and formed in the reaction.

For each reaction, calculate the total enthalpy change by subtracting the total bond enthalpy of the bonds broken from the total bond enthalpy of the bonds formed: (a) ΔH(a) = Σ Bond enthalpies of bonds formed in the products - Σ Bond enthalpies of bonds broken in the reactants (b) ΔH(b) = Σ Bond enthalpies of bonds formed in the products - Σ Bond enthalpies of bonds broken in the reactants (c) ΔH(c) = Σ Bond enthalpies of bonds formed in the products - Σ Bond enthalpies of bonds broken in the reactants

After calculating the enthalpy changes for each reaction using the data from Table 8.4, report the values for ΔH(a), ΔH(b), and ΔH(c). These values represent the estimated enthalpy change for each reaction.