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- Which of the following is one of several products that could result from the reaction conditions shown? (Note: There are many products that could result under these conditions, however only one of the choices below is one of those possibilities). OH H2SO4 HO, (A) (B) (C) (D) O A ов OC ODOH H₂SO4 cat. SN2 conditionsBr NaOH DMF (H2O) S OH Br ОН Ь ОН ОН 3.
- I2 (aq) + CH3COCH3 (aq) HI (aq) + ICH2COCH3 (aq)Iodine in solution has a yellow-brown color, whereas the acetone and both products are colorless. This means that we can run the reaction using iodine as the limiting reagent, and when we see that the yellow-brown color of the iodine has disappeared, we know that the reaction has stopped and all of the iodine has been consumed. Recall that to calculate a rate of reaction, we would like toknow the change in concentration of a reactant or product during a fixed amount of time. Wewill choose the reactant iodine in this case, because its brown color allows us to determinewhen its concentration has fallen to zero. Rate = –Δ[I2] / Δt = – ([I2]final – [I2]initial) / ([tfinal – tinitial) = – (0 – [I2]initial) / (tfinal – 0) = [I2]initial / tfinal Run several trials at different concentrations of reactants and use themethod of initial rates to obtain values for k, x, y, and z in the rate law. Rate = k [I2]x [acetone]y [H+]z Run the…I2 (aq) + CH3COCH3 (aq) HI (aq) + ICH2COCH3 (aq)Iodine in solution has a yellow-brown color, whereas the acetone and both products are colorless. This means that we can run the reaction using iodine as the limiting reagent, and when we see that the yellow-brown color of the iodine has disappeared, we know that the reaction has stopped and all of the iodine has been consumed. Recall that to calculate a rate of reaction, we would like toknow the change in concentration of a reactant or product during a fixed amount of time. Wewill choose the reactant iodine in this case, because its brown color allows us to determinewhen its concentration has fallen to zero. Rate = –Δ[I2] / Δt = – ([I2]final – [I2]initial) / ([tfinal – tinitial) = – (0 – [I2]initial) / (tfinal – 0) = [I2]initial / tfinal Run several trials at different concentrations of reactants and use themethod of initial rates to obtain values for k, x, y, and z in the rate law. Rate = k [I2]x [acetone]y [H+]z Run the…H;CO A B H. E D