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- Does increasing the amount of a reactant (NOT THE CONCENTRATION) from say 2.5mL to 5.0mL of Na2S2O3 increase the rate of a reaction or lower it?Sketch an energy diagram for a two-step reaction in which both steps are exergonic and in which the second step has a higher-energy transition state than the first. Label the parts of the diagram corresponding to reactant, product, intermediate, overall AG+, and overall AG°.Which of the four reactions does NOT proceed through the same intermediate as the others?
- 5. If a reaction mechanism produces a stable intermediate, would you expect to be able to start from that intermediate (instead of the starting material) in order to form the desired product? Explain.The following reaction proceeds at a rate such that 4 mole of AA is consumed per minute. Given this, how many moles of CC are produced per minute? 2A+2B→4CWhich step is the rate-determining step of the reaction?
- What are the intermediates of the following reaction?According to this reaction energy diagram, the value of the change in energy is. Potential energy (kJ/mol) A ヨ ԱՄ B D C Reaction progress positive negative greater than the energy of the reactants greater than the transition state energyDetermine and draw the intermediate (X) for the following reaction. HINT: this is not an S,2 reaction. KCN CN H,0, heat
- Which of the following statements is TRUE regarding the energy profile shown below? in Reaction Progress O The reverse reaction is faster than the forward reaction. The reaction mechanism involves one transition state, two intermediates, and one catalyst. O The forward reaction is a catalyzed reaction with E₂ < 0. The reaction proceeds via a two-step mechanism where the 2nd step is the rate determining step. EnergyHydrogen peroxide is a common household chemical. Is it likely that the decomposition of H2O2 proceeds at a fast rate without a catalyst? yes noProducts Reactants Extent of reaction Which letter shows the non-catalyized reaction? Energy