Consider the following reaction mechanism. k1 C2H6O(aq) + HCI(aq) 5 C2H¬O*(aq) + Cl'(aq) k-1 (fast, reversible) k2 CH;O*(aq) + Cl(aq) → C2H5CI(aq) + H20(1) (slow) a) Write the overall reaction that is indicated by the mechanism. b) Are there any reaction intermediates? If so, identify them. c) Is there a catalyst? If so, identify it. d) What is the rate law for this mechanism?

A+OHA+H₂O O₂ (g) ⇒ 0₂ (soln) O₂ (soln) + X⇒ B B + A⇒X+ products (fast equilibrium) (fast) (fast) (slow) Show that the observed rate law: d[products]/dt = kobs[B][A][OH]. Include step-by-step solution.

1) The rate constant for the gas-phase reaction H2(g) + I2(g) → 2 HI(g) has the value 4.45 x 10-5 mol-1 dm³ s-1. What is the equivalent rate constant in units of molecule-1 cm³ s- 1? 2) The kinetics of the hydrolysis of methyl methanoate, CH3COOCH3, in aqueous solution were investigated by measuring the concentration of the ester after different time intervals. The reaction was found to be first order in the concentration of the ester. Use the data below to determine the rate constant for the reaction (must provide best fit graph). 3600 time, t/s 1800 5400 7200 9000 concentration, c/ (mol dm-3) 0.300 0.191 0.135 0.081 0.055 0.035

10. The rate of change in colour of iodide (yellow) can be measured as it reacts with colourless hypochlorite, OCI (ag): I (aq) + OCI(aq) I0- (aq) + Cl (aq) a. Different concentrations of reactants are combined at the same temperature and the rate of yellow colour disappearance were measured: Rate of colour Trial Initial [I] (mol/L) Initial [OCI(ag)) change (mol/(L s) 0.12 0.18 7.91 x 102 1 0.18 3.95 x 102 0.060 0.090 0.030 9.88 x 103 3 0.24 7.91 x 102 4 0.090 Using the data provided, calculate the value of the rate constant, including units b. Predict the rate of reaction if both reactants have an equal starting concentration of 0.10 mol/1.

Write down the kinetic equation for a simple reaction in a homogeneous medium 2A + B = 2C. Indicate the general and in relati on to all reactants reaction orders

2C4H6(g) → C8H12(g) At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The rate of the reaction was studied at 625 K in a rigid reaction vessel. Two different trials, each shown with a different starting concentration, were carried out. The data were plotted in three different ways, as shown below. (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all  the gas present in the vessel is C4H6. (Hint-this is a gas law problem from chemistry last year) (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6. (c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for  the reaction at 625 K.

Consider the following proposed reaction mechanism: (1) CIO (aq) + H,O(1)= HCIO(aq) + OH (aq) [fast] (2)I (aq) + HCIO(aq) → HIO(aq) + Cl¯(aq) [slow] (3) OH (aq) + HIO(aq) → H,O() + 10 (aq) [fast] Ignoring water, how many reaction intermediates are present? O 3 O 1 O 2

For a simple reaction, S 1 P, k1 is the rate of the forward reaction and k-1 is the rate of the backwards reaction.  The k1 in the absence of any enzyme was 0.01/s.  The k1 in the presence of enzyme was 5,000,000/s. Calculate the rate enhancement (k1 catalyzed divided by k1 uncatalyzed) provided by the enzyme. If the equilibrium constant in the absence of enzyme is 1 x 104, what is the equilibrium constant (Keq) in the presence of enzyme?

0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H*]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H* = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HI

The reaction described by the following equation: 21-(aq) + H;O2(aq) + 2H*(aq) → I:(aq) + 2H;O(aq) has an experimental rate law (v) = k[I][H2O2]. Suggest a plausible mechanism for this reaction, and identify the rate-determining step.