Save Answer In an endothermic single step reaction, the transition state is a late transition state. In this case, the transition state does not resembles structurally the product of the reaction O True O False

When the concentration of reactant molecules is increased, the rate of reaction increases. The best explanation is: As the reactant concentration increases,     the rate constant increases.     the activation energy increases.     the frequency of molecular collisions increases.     the order of reaction increases.     the average kinetic energy of molecules increases.

provide full reaction mechanism and state where the equilibrium shifts

True or false The rate limiting step in a reaction is the slowest step in the reaction sequence.

What is the appropriate reaction intermediate or transition state (whichever is applicable) for this reaction? H s H [] **** OCHS ********* H Br O NaOCH3 OCH

As the temperature of a reaction is increased, the rate of reactions increase because the CA. reactant molecules collide less frequently OB. activation energy is lowered C. reactant molecules collide with greater energy D. reactant molecules collide less frequently but with greater energy OE. activation energy is increased

The exergonic reaction below involves multiple elementary steps and one of the intermediates in the reaction is shown in square brackets. Which statement is consistent with this reaction? HCI, H2O но OH O This is a rearrangement reaction O The low energy transition state makes the reaction exergonic O The reaction has at least two transition states and the products are lower in energy than the reactants O The intermediate in the reaction must be more stable than the reactants O The reaction has one transition state, and the products are lower in energy than the reactants

Label the energy diagram (7 bins) and indicate which reaction corresponds to the energy diagram. rate-limiting Answ transition state non-limiting transition state activation energy intermediates products starting AG° materials reaction coordinate energy 00

Which of the four reactions does NOT proceed through the same intermediate as the others?

2NO2(g) + F2(g) -> NO2F(g) H°rxn = -284 kJ/molrxn NO2(g) and F2(g) can reactto produce NO2F(g), as represented above. A proposed mechanism for the reaction has two elementary steps, as shown below. Step 1: NO2 + F2 -> NO2F + F          (slow) Step 2: NO2 + F -> NO2F         (fast) a.) Write a rate law for the overall reaction that is consistent with the proposed mechanism. b.) On the incomplete reaction energy diagram below, draw a  curve that shows the following two details. The relative activation energies for the two elementary steps  The enthalpy change of the overall reaction    Can all of them be solved please, and thank you very much!