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(B) The equilibrium constant for hydration depends on the electrophilicity of the carbonyl carbon and steric hindrance.$1$. Aldehydes are more reactiv

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$A < C < B < E < D$

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(B) The equilibrium constant for hydration depends on the electrophilicity of the carbonyl carbon and steric hindrance.$1$. Aldehydes are more reactive than ketones due to less steric hindrance and lower electronic stabilization of the carbonyl carbon.$2$. Electron-withdrawing groups (like $-Cl$) increase the electrophilicity of the carbonyl carbon,thereby increasing the equilibrium constant for hydration.Comparing the compounds:$(A) CH_3COCH_3$ (Ketone,no $-I$ group)$(B) CH_3CHO$ (Aldehyde,no $-I$ group)$(C) ClCH_2COCH_3$ (Ketone with $-I$ group)$(D) HCHO$ (Smallest aldehyde,no $-I$ group)$(E) ClCH_2CHO$ (Aldehyde with $-I$ group)Order of reactivity:Ketones: $(A) Aldehydes: $(B) Combining these,the increasing order is: $(A) < (C) < (B) < (E) < (D)$.

Arrange the following compounds in increasing order of their equilibrium constants for hydration:
$(A). CH_3COCH_3, (B). CH_3CHO, (C). ClCH_2COCH_3, (D). HCHO, (E). ClCH_2CHO$

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Arrange the following compounds in increasing order of their equilibrium constants for hydration:$(A). CH_3COCH_3, (B). CH_3CHO, (C). ClCH_2COCH_3, (D). HCHO, (E). ClCH_2CHO$