Sort the following elementary reactions as unimolecular (1), bimolecular (2) or termolecular (3) and write down the rate law expression for that step Elementary step from reaction mechanism Molecularity Rate law for elementary step (CH3)3CBr → (CH3);C* + Br 2NO2 → N2O4 CH3CI +I → CH31 + Cl

Consider the following reaction mechanism for the addition of HCl to propene in the gas phase. The overall reaction is just HCI + CH3CH=CH2 → CH;CH2CH3, but the experimentally observed rate law is more complicated than that stoichiometry would suggest. 2 HCl 2 (HCI), k_1 k2 HCI + CH3CH = CH, 2 complex k_2 (HCI)2 + complex → CH3CHCICH3 (Here (HCl)2 is an HCl dimer and “complex" represents some intermediate species of unknown structure.) Assume that the third step is rate determining, and that the first two steps both remain in equilibrium throughout the reaction. d[CH;CHCICH3] Please write Derive an expression for the rate of formation of CH3CHCICH,' dt your final expression in the boxes. HINT: Be sure to use the equilibrium assumption, and not the steady state approximation. Your final rate law should NOT include the concentrations of any intermediates.

Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A + 2B-C+D k= esc @ NO 2 # 3 с Ad 4 % Trial [A] (M) [B] (M) Rate (M/s) 1 0.250 0.200 2 0.250 0.400 3 0.500 0.200 5 Units G Search or type URL MacBook Pro A 6 & 7 0.0168 0.0168 0.0672

Using the data in the table, determine the rate constant of Trial [A] (M) [B] (M) Rate (M/s) the reaction and select the appropriate units. 1 0.280 0.200 0.0163 A +2B C+ D 0.280 0.400 0.0163 0.560 0.200 0.0652 Units k =

Given the following results: Rate of Run Reaction [1] (M/s) 1.76 0.358 0.476 4.72 0.358 0.843 5.25 0.672 0.476 1 2 3 [H₂O2] Calculate the rate constant(k) for each run. Assuming the Rate Law = k[1]²[H₂O₂] calculate the average rate constant,k, for this reaction. Give your answer to 2 places after the decimal.

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We are determining the rate law equation for a reaction A + B + C > ABC in which a dramatic and instant color change tells us that reactants are used up and product is formed. (Concentrations used in all experiments are [A] = 2.0M, [B] = 1.0M and [C] = 3.0M) This is the data for questions 19 through 22: Volume of Volume of water, C, Volume of Volume of Time from mixing to dramatic color А, B, ml change, sec ml ml ml 1.0 1.0 1.0 97.0 16 1.0 1.0 2.0 96.0 8 19) Which reactant concentration have we changed? a) A b) B c) C d) no reactant concentrations changed

Propose a reaction pathway consisting of only a unimolecular or bimolecular steps for the 2A+B-->C+D that is consistent with the rate law rate=k(A)(B). Make sure you label which step is the rate determining step and prove that your proposed mechanism gives both the overall reaction and overall rate law. Explain the assumptions you must make in order for your mechanism to be consistent with the actual rate law.

The overall gas phase reaction  3A --> B + 2C occurs via the following sequence of elementary steps 2A <--> I1 + B    k1,k2 A + I1 --> 2I2        k2 I2 --> C               k3 1. write an expression for the overall reaction rate, r, in terms of the rate step 3, r3 2. using the answer from 1, obtain an expression for the reaction rate, r, in terms of rate constants and concentrations of reactants and products, only use PSSH. 3. State the. specific inequality the must be satisfied for each of the following assumptions to hold, and use it to simplify the general rate expression from question 2.         i) Step 1 is quasi-equilibrium         ii) Step 1 is irreversible

Given the following data, determine the rate constant (in M-2s-1) of the reaction 2NO(g) + Cl2(g) –→ 2NOCI(g) [Cl2] (M) Rate (M/s) 3.4 x 104 8.5 x 105 3.4 x 104 Experiment [NO] (M) 1 0.0300 0.0100 0.0150 0.0100 3 0.0150 0.0400 Note: Answers must be numeric, not alphanumeric-42, not forty-two.