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(A) Reaction $A$ represents an $S_N2$ mechanism involving a neutral nucleophile and a neutral substrate,leading to a charged transition state. Increas

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Increase in both $A$ and $B$

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(A) Reaction $A$ represents an $S_N2$ mechanism involving a neutral nucleophile and a neutral substrate,leading to a charged transition state. Increasing solvent polarity stabilizes the charged transition state more than the reactants,thus increasing the rate.Reaction $B$ represents an $S_N1$ mechanism where the rate-determining step involves the formation of a carbocation $(R^{+})$ and an anion $(L^{-})$. Increasing solvent polarity stabilizes the ionic transition state and the resulting ions,thereby increasing the rate of reaction $B$ as well.

What would be the effect of increasing solvent polarity on the rate of each of the following reactions? ($Nu =$ neutral nucleophile)
$A. Nu + R-L \to Nu^{+}-R + L^{-}$
$B. R-L \to R^{+} + L^{-}$

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What would be the effect of increasing solvent polarity on the rate of each of the following reactions? ($Nu =$ neutral nucleophile)$A. Nu + R-L \to Nu^{+}-R + L^{-}$$B. R-L \to R^{+} + L^{-}$