Question
Use bond energies (Table 8.4) to predict $\Delta H$ for the isomerization of methyl isocyanide to acetonitrile:$$\mathrm{CH}_{3} \mathrm{~N} \equiv \mathrm{C}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{C} \equiv \mathrm{N}(g)$$
Step 1
According to Table 8.4, the bond energies are as follows: - C-H: 413 kJ/mol - C≡N: 891 kJ/mol - C-N: 293 kJ/mol Now, we need to form the bonds in acetonitrile (CH3-C≡N). The bond energies are: - C-H: 413 kJ/mol - C≡N: 891 kJ/mol - C-C: 347 kJ/mol Show more…
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Use bond energies (Table 8.5$)$ to predict $\Delta H$ for the isomerization of methyl isocyanide to acetonitrile: $$\mathrm{CH}_{3} \mathrm{N} \equiv \mathrm{C}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{C} \equiv \mathrm{N}(g)$$
Use bond energies to predict $\Delta H$ for the isomerization of methyl isocyanide to acetonitrile. $$ \mathrm{CH}_{3} \mathrm{N} \equiv \mathrm{C}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{C} \equiv \mathrm{N}(g) $$
Use bond energies (Table $3-3$ ) to predict $\Delta E$ for the isomerization of methyl isocyanide to acetonitrile: $$ \mathrm{CH}_{3} \mathrm{N}=\mathrm{C}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{C}=\mathrm{N}(g) $$
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