Substrate A Br Br Substrate B Br Br Br Faster Rate (Choose one) Substrate A Substrate B Roughly Equal Rate (Choose one) (Choose one) Y

What amount of catalyst is necessary to significantly change the reaction rate of peroxide hydrogen decomposition? O A catalyst does not influence the rate of reaction O Equal to hydrogen peroxide O Half of hydroxide peroxide O Small DD 000 החמ F9 F10

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Step 1)   X(g) + Y(g)   A(g)   fast, reaches equilibrium (For Step 1,  k1 = forward rate constant & k-1 = reverse rate constant.)Step 2) A(g) + Z(g)   B(g)    slow  (k2 = rate constant) Step 3)  B(g)   P(g)   fast  (k3 = rate constant) a) What is the overall reaction?   b) What is the rate law supported by this mechanism?  Explain your answer.  c) The following is experimental data found for this reaction:    Initial [X] (M) Initial [Y] (M) Initial [Z] (M) Initial Rate   (M/day) Exp 1 0.150 0.150 0.150 0.569 Exp 2 0.250 0.150 0.150 0.948 Exp 3 0.250 0.300 0.150 3.793 Exp 4 0.300 0.350 0.200 6.196      i) What is the experimentally determined rate law?       ii) Determine the rate constant and include units.    d) Does your experimentally determined rate law support the proposed mechanism?  Explain your answer.   e) ΔΔHo = -347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed mechanism. Label your profile with the proper reactants,…

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

1. What is the difference between a transition state and an intermediate?

In comparing these two reactions, which one would occur faster via the SÃ2 mechanism and why? Reaction I CI OH- Reaction II CI 1 NH₂

Consider the following reaction and predict the new rate of the reaction if the concentration of A is doubled and the concentration of B was quadrupled.  The new rate will be how many times greater than the original rate?

Another common component of reaction mechanism is a catalyst. These are compounds that change the reaction mechanism and provide a pathway with a lower activation energy, and correspondingly faster reaction rate. They are a reactant in an early step in the mechanism and a product in a later step. They do not appear in the overall reaction but do appear in the rate law. 3. A reaction occurs by the following mechanism; Step 1 Ce4+ + Mn²+ →→ Ce³+ + Mn³+ Step 2 Ce4+ + Mn³+ → Ce³+ + Mn²+ Step 3 Tit+ Mn+→ Ti³+ + Mn²+ a. Write the overall reaction. b. Identify each of the components as a reactant, product, intermediate, or catalyst; Mn²+ Mn³+ Ce4+ Ce ³+ Mn4+ Tit Ti³+ C. Assuming that the catalyst is involved in the rate determining step, what is the rate law for this reaction? 4. Under certain conditions, the reaction: 2 NO + Cl₂ → 2 NOCI is found to be second order in NO and first order Cl₂. Given the following mechanism; Step 1 NO + Cl2 → NOCI₂ Step 2 NOCI₂ + NO 2 NOCI a. What are the…