Answer
the isomerization of methyl isocyanide to acetonitrile is an exothermic reaction, with a decrease in energy of 43 kJ/mol.
Work Step by Step
To predict the change in energy (ΔE) for the isomerization of methyl isocyanide to acetonitrile, we can use the bond energies provided in Table 3-3.
The reaction can be represented as:
$CH_{3}N=C(g) \rightarrow CH_{3}C\equiv N(g)$
To calculate the ΔE, we need to consider the bond energies of the bonds that are broken and formed during the reaction.
Bonds broken:
- C-N bond in methyl isocyanide: 305 kJ/mol
Bonds formed:
- C-C bond in acetonitrile: 348 kJ/mol
The change in energy (ΔE) can be calculated as:
ΔE = Bonds broken - Bonds formed
ΔE = 305-348
ΔE = -43 kJ/mol
Therefore, the isomerization of methyl isocyanide to acetonitrile is an exothermic reaction, with a decrease in energy of 43 kJ/mol.
