A 2-step reaction has the following mechanism: | 1. (fast) R2 R+R 2. (slow) R+Q K₂ P k_1 What series does it have? (A). v= - = (k + k1 − k-1)[R2][Q] (B). v=-k₁[R₂] + k₁[R]² - k₂[R][Q] (C). v=k₂[R]²[Q]² (D). v = k[R₂]1/2[Q]

For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.

AKB KC KD If the rate-determining step is the second step (B = C), indicate the acceptable option. (A). K2 must be exactly equal to K-2 (B). K₂ ≈ k3 (C). K3 << k2 y k3 << K-2 (D). K₂ << K-1

The proposed 3-step mechanism for a reaction is Step 1) X(g) + Y(g) A(g) fast, reaches equilibrium (For Step 1, k1 = forward rate constant & k.1 = reverse rate constant.) %3D Step 2) A(g) + Z(g) Step 3) B(g) B(g) slow (k2 = rate constant) 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] Initial [Y] Initial [Z] Initial Rate (M) (M) (M) (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) AH° = +347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed mechanism. Label your profile with the proper reactants, products,…

Given the transition state diagram(s) below, identify the mechanism(s) of catalysis. Mg2+ Mg2+ H OH H-C-H HOH H H - (M₂C)N= H H-C-H HO -H H- HO -H OH-O -O-H- H-N(CH₂) CH₂OH H H₂C H H LN (CH2) H OH HOH:N (0³H)² CH₂OH H₂C t

What would the orientation factor be for this reaction? Why? (>1, <1, or =1)

Q5: Write rate laws that would describe the rate of product formation for the following system

The reaction of CH;OH and HBr is believed to proceed by the mechanism: ki CH:OH +H+ = CH:OHz* k1 Elementary Step 1: (Fast pre-equilibrium) Elementary Step 2: k2 CH;OH2* + Br- 5 CH;Br + H2O (Slow) (а) What is the stoichiometric overall equation for the reaction? (b) What is the intermediate in the proposed mechanism? (c) Derive the rate law predicted by this mechanism. Show your working out.

How is ΔG related to the forward (k1) and reverse(k-1) rates of a reversible first order reaction?                                                                               ΔG = -RTln(k1/k-1) (k-1/k1) = e(-ΔG/RT)  k1/k-1) = -e(ΔG/RT) ΔG = RTln(k1/k-1)

The rate law of the elementary reversible reaction CO + 2H2 < - > CH3OH is k [ Cco CH2 - K CcH3OH ) is True or False Multiple choise