If CII3 COOII+OII ⟶CII3 COO+H2 O+q1 and II^++O II →II2 O+q2, then enthalpy change for the reacti

step 1 If acetic acid plus hydroxyl group forms acetate plus water plus Q1 and hydrogenine plus hydroxy

If CII3 COOII+OII ⟶CII3 COO+H2 O+q1 and II^++O II →II2 O+q2,...

If $\mathrm{CII}_{3} \mathrm{COOII}+\mathrm{OII} \longrightarrow \mathrm{CII}_{3} \mathrm{COO}+\mathrm{H}_{2} \mathrm{O}+\mathrm{q}_{1}$ and $\mathrm{II}^{+}+\mathrm{O} \mathrm{II} \rightarrow \mathrm{II}_{2} \mathrm{O}+\mathrm{q}_{2}$, then enthalpy change for the reaction $\mathrm{CH}_{3} \mathrm{COOH} \longrightarrow \mathrm{CH}_{3} \mathrm{COO}+\mathrm{H}^{+}$ is equal to (1) $\mathrm{q}_{1}+\mathrm{q}_{2}$ (2) $\mathrm{q}_{1}-\mathrm{q}_{2}$ (3) $\mathrm{q}_{2}-\mathrm{q}_{1}$ (4) $-\mathrm{q}_{1}-\mathrm{q}_{2}$

If $\mathrm{CII}_{3} \mathrm{COOII}+\mathrm{OII} \longrightarrow \mathrm{CII}_{3} \mathrm{COO}+\mathrm{H}_{2} \mathrm{O}+\mathrm{q}_{1}$
and $\mathrm{II}^{+}+\mathrm{O} \mathrm{II} \rightarrow \mathrm{II}_{2} \mathrm{O}+\mathrm{q}_{2}$, then enthalpy change for
the reaction $\mathrm{CH}_{3} \mathrm{COOH} \longrightarrow \mathrm{CH}_{3} \mathrm{COO}+\mathrm{H}^{+}$ is equal to
(1) $\mathrm{q}_{1}+\mathrm{q}_{2}$
(2) $\mathrm{q}_{1}-\mathrm{q}_{2}$
(3) $\mathrm{q}_{2}-\mathrm{q}_{1}$
(4) $-\mathrm{q}_{1}-\mathrm{q}_{2}$

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Key Concepts

Hess's Law

This principle states that the total enthalpy change for a chemical reaction is independent of the pathway taken, meaning that it can be determined by summing the enthalpy changes of multiple steps that add up to the overall reaction.

Reaction Enthalpy

Reaction enthalpy refers to the net heat absorbed or released during a chemical reaction. It is a key aspect in thermochemistry and can be measured experimentally or computed by using thermochemical equations and Hess's Law.

Thermochemical Equations

These are balanced chemical equations that include the enthalpy changes associated with the reactions. They provide a framework to analyze complex reaction pathways by breaking them down into simpler steps with known enthalpy values.

Acid Ionization

This concept involves the dissociation of an acid into its conjugate base and a proton. Understanding the enthalpy change of acid ionization requires applying thermochemical principles such as Hess’s Law and the combination of enthalpy changes from related reactions.

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