What happens to the rate of an SN2 reaction under the following conditions? [RX] is halved, and [:Nu−] is doubled.

The rate of the following reaction is dependent on the concentration of: Br + NaN3 DMF N3 + NaBr

Consider a reaction taking place in an aqueous solvent. The transition state for this reaction is capable of interacting more strongly with the aqueous solvent (through low potential energy interactions, including hydrogen-bonding) than with the reactant/ground state. Despite these strong potential energy interactions, the reaction rate is not significantly faster than the same reaction taking place in a non-polar solvent. Why? a)The transition enthalpy is unchanged by the aqueous solvent b)The transition Gibbs energy is reduced in the aqueous solvent c) The transition entropy is significantly negative in the aqueous solvated reaction d) The transition state internal energy is significantly negative in the aqueous solvated reaction d) none of the above

What are two sets of reaction conditions that could be used?

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VI. The rate of the reaction (CH3)3CCI + NaSCH2CH3 → (CH3)2C=CH2 + CH3CH2SH + NaCl is first-order in (CH3)3CCI and first-order in NaSCH₂CH3. Please draw the rate- limiting step of the reaction, using curved arrows to show the flow of electrons. If any lone pairs are involved in a reaction, their involvement must be explicitly shown. ( 20