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- i. Which of the reactions given below is wrong? H3O*/H20 (A) MgBr + CO2 H2/Pt (B) CH;CH2CN CH;CH,NH2 heat NABH4 (C) HO OH/H20 (D) CI OHTranslate the following reaction completely into English words using no symbols: 4NH3 + 5O2 --> 4NO + 6H2O4b give the product if it gives reaction, if not, write no reaction
- 27) Draw the chemical structure of the products of the following reactions. " Pt " HO + 2 H2 K2S(aq) Pb(NO3)2(aq) OH HO. + Cu+2 H- Но H- ČH2OH H2N. H30* HO, NHProvide the products for the following reactions: + + MeO2C .CO₂MeWhat is the main product of these reactions (a) (c) CI 44 2 NaNH,, liq. NH Equivalent (b) Qatçı (d) NaOCH3, CH₂OH (D) CO C 3 NaNH,, liq. NH Equivalent NaOCH3, CH₂OH
- Draw the organic product expected from the reaction. Include all hydrogen atoms. Note that K, Cr, 0, is present in excess. H H H, SO, CH, CH,CH, OH + K,Cr,0,(aq) |Provide the product(s) produced in the following reaction: 0=8=0 KOHProvide the major product for the following reaction? (1) Mg, ether (2) CO2. (3) H3O* Br
- (ii) Identify the major products in the following reactions a) 200 °C 200 °C b) X + Y c) 180 °CI2 (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…