The following question was asked in one of the assignments my teacher has given.
Acetone ($\ce{Me2CO^16}$) on treatment with $\ce{H2O^18}$ gives a mixture of $\ce{Me2CO^16}$ and $\ce{Me2CO^18}$, the latter being in slight excess. This may be explained by
(A) hydration of acetone is an equilibrium process
(B) $\ce{C – O^18}$ bond is slightly stronger than $\ce{C – O^16}$
(C) $\ce{Me2CO^18}$ forms stronger hydrogen bonds than $\ce{Me2CO^16}$ with water
(D)hydration of acetone is irreversible
I have doubt about option (C). According to me, (C) should be correct, but it is given incorrect. Why the $\ce{^18O...H}$ is weaker than $\ce{^16O...H}$ bonding?