The clock reaction reaction: H2O2 + 3I- + 2H+ → I3- + 2H2O occurs through the following mechanism.                                                                                H2O2 + H+ ↔ H3O2+ (fast equilibrium K1 ) H3O2+ + I- → H2O + HOI  (slow k2 )  HOI + I- → OH- + I2           (fast k3) OH- + H+ → H2O (fast  k4) I2 + I- → I3- (fast k5) What is the rate law for this reaction?

The rate of a reaction is increased with the addition of a catalyst as shown in the following diagram: Praducts Reactants Reaction Coordinate Energy

The following mechanism is proposed: C6H5COOH ⇌ C6H5CO2H2+   (fast) C6H5CO2H2+ ⇌ C6H5CO+ + H2O   (fast) C6H5CO+ + HX + H2O ⟶ C6H6NH2 + N2 + CO2  (slow) The overall enthalpy change is -237.6 kJ. Sketch a reaction-energy diagram consistent with the above mechanism and the enthalpy change. Label the enthalpy change and each transition state. Explain the appearance of your graph.

Assuming both reactions are at the same temperature, Which one would produce product faster?   II Both would produce product at the same rate   Not enough information to tell I

A certain reaction is known to proceed slowly at room temperature. Is it possible to make the reaction proceed at a faster rate without changing the temperature?

Consider the following reaction mechanism. Step 1 : W2  ⇌ 2W                 (fast) Step 2 : W + Z ⇌    D +  F       (fast) Step 3 : W + F  →     M           (slow)What are the intermediates?

Classify the actions based on how they could affect a reaction rate. Rate increases Rate decreases Rate is unaffected Answer Bank decrease the concentration of a reactant decrease the surface area of a solid reactant increase the temperature add a catalyst

7. Reactions A and B were studied and found to produce the given energy diagrams. 150 150 Energy 100 (kJ/mol) 100 Energy (kJ/mol) 50 50 Reaction progress Reaction progress Reaction A Reaction B A third reaction, C was studied with a measured activation energy of 55 KJ/mol. Assume all reactions take place at the same temperature. Reaction A is slowest a. b. Reaction B is slowest c. Reaction C is slowest d. All reactions happen at the same rate.

ic) (a) Reaction coordinate X+Y - 2) What is represented by the letter (e) in the diagram above? the potential energy of the activated complex the activation energy (Ea) of the forward reaction the potential energy of the products the potential energy of the reactants

At equilibrium, the mechanism 2 The reaction, A + 3B-> D + F was studied and the following mechanism was established: A + B -> C (fast) C + B-> D+E (slow) E + B > F (very fast) W #3 Peaction rate equals the reverse reaction rate. E $ 4 R % 5 T MacBook Pro 6 Y & 7 The species E is properly described as a co-factor an intermediate a reactant an enzyme a catalyst The species C is properly described as a catalyst an enzyme an intermediate a co-factor a reactant U 8 ( n O