Question

Using the bond energies provided, calculate the enthalpy of the reaction (∆HRxn, in kj) for the industrial synthesis of rubbing alcohol shown below. CH₃CHCH₂(g) + H₂O(l) → CH₃CH(OH)CH₃(l)

Answer 1

To calculate the enthalpy change for the synthesis of rubbing alcohol, we would subtract the energy of bonds formed in the products from the energy of bonds broken in the reactants.

Step-by-step explanation:

To calculate the enthalpy of the reaction (ΔHRxn) for the synthesis of rubbing alcohol (CH3CH(OH)CH3), you must consider the bond energies of the reactants and products. The process involves breaking the bonds in the reactants and forming new bonds in the products. However, since the specific bond energies are not provided, we would normally use given bond energies to calculate the total energy needed to break the bonds of the reactants and the energy released when the new bonds in the products are formed. The difference between these energies would give you the approximate enthalpy change of the reaction.

For instance, if you were provided the bond energies in a table, you would subtract the energy of the bonds formed in the products from the energy of the bonds broken in the reactants. This calculation gives you an approximation of the enthalpy change, which can indicate if the reaction is exothermic (releases heat) or endothermic (absorbs heat). Examples of such calculations show that if the bonds in the products are stronger, then the reaction usually releases more energy than it consumes, resulting in an exothermic reaction as seen in similar reactions where ΔH was calculated using bond energies.