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- How many unique products are produced in the reaction shown? O 1 O 2 O 3 O 4 1) xs LIAIH4 2) H₂OPredict the product(s) of the following reaction. Br I A I B || C D) I, II E) I, II, III, IV Br BI || HBr = ||| ? Br IV BrTranslate the following reaction completely into English words using no symbols: 4NH3 + 5O2 --> 4NO + 6H2O
- 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 ODAt the beginning of a reaction, there is virtually no product. O True O FalseIn this reaction, the limiting reagent is Question 6 options: None AlBr3 Al Br2 H2O
- Which statement best describes the products of this reaction?Considering each of the following values and neglecting entropy, tell whether the starting material or product is favored at equilibrium: (a) ΔH° = 80 kJ/mol; (b) ΔH° = −40 kJ/mol.3. Predict the products of the following halogenation reactions. OH Br₂, hv HBr HBr ROOR PBr3
- how H2O2 can be prepared on the large scale?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…A kinetically-controlled process describes a reaction that. O generates the most stable product O generates the product whose formation requires the smallest energy of activation O generates the product requiring the fewest steps O generates the product formed at the slowest rate O generates the product favored at high temperatures