The following mechanism has been suggested for the reaction between chlorine and chloroform: Cl2 (g) + 2Cl (g), K₁, fast CHCl3 (8) + Cl (g) → CC13 (g) + HCl (g), k2, slow CC13 (8) + Cl (g) → CCl4 (g), k3, fast The rate law for this mechanism is controlled by: Rate2= K₂ [CHCl3] [CI] Rate₁ = K₁ [Cl₂] Rate.1= K.1 [CI]² Rate3 K3 [CCI3] [CI]

Consider the mechanism: NO2(8) + SO2(g) → NO(g) + SO3(g) NO(g) + ½ O2(g) –→ NO2(g)

Consider the mechanism. O3 + NO, – NO, + O, NO, + NO, – N,O5 slow fast O, + 2 NO, – 0, + N,O5 Identify the rate law for the overall reaction based on the mechanism. rate = k[O,||NO,? rate = k[O3] rate = k[O3][NO,1 rate = k[NO,? k[NO, ][NO3] rate =

Nitrogen Pentoxide Decomposition Consider the decomposition of nitrogen pentoxide into nitrogen dioxide and oxygen, N2O5 → 2 NO2 + ½ O2 R1 This is not an elementary reaction and its mechanism consists of the following set of elementary reactions. N2O5 → NO3 + NO2                        R1a NO2 + NO3 → N2O5                         R1b NO2 + NO3 → NO2 + O2 + NO         R1c NO + NO3 → 2NO2                            R1d The rate constants for the reactions R1a, R1b, R1c and R1d are denoted as k1, k2, k3 and k4, respectively. Here, NO and NO3 are regarded as the intermediate species. (a) Derive the rate expression for the overall reaction R1 from its mechanism (R1a-d) using the pseudo- steady state approximation. (b) What is the overall order of the reaction? Explanation: Pseudo steady state is similar to the rate determination done for catalytic reactions

The following mechanism has been proposed for the reaction of H2 (g) and NO (g): H2 (g) + NO (g) → H2O (g) + N (g) (Slow)N (g) + NO (g) → N2 (g) + O (g) (Fast)H2 (g) + O (g) → H2O (g) (Fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.

The following mechanism has been proposed for the atmospheric decomposition of nitric oxide (NO). Step 1: 2 NO (g)  N2O Step 2: 2 (g)N2O2 (g) + H2 (g)  N2O(g) + H2O(g) Step : N2O(g) + H2 (g)  N2 (g) + H2O(g) Identify any intermediates in this reaction mechanism. Write the overall chemical reaction. Sketch the energy diagram for Step 1. E = - 4 kJ/mole. Include axes with labels. Label the reactants, product, and transition state on the energy diagram. Write the differential rate law for Step 1

Consider this reaction: 2C1,0, g) → 2C1, (6) + 50, (g) At a certain temperature it obeys this rate law. rate = (0.36 Ms)[C1,0,1 %3D Suppose a vessel contains Cl,0, at a concentration of 0.630 M. Calculate how long it takes for the concentration of Cl,0, to decrease to 5.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.

Consider the reaction for the formation of ammonia, NH3:                              N2(g) + 3 H2(g) --> 2 NH3(g) Which is the correct rate expression for this reaction?

Writing the rate law implied by a simple mechanism with an initial slow... Suppose the formation of nitryl fluoride proceeds by the following mechanism: elementary reaction step 1 NO₂ (g) +F₂ (g) 2 k₁ k₂ 2 F (g) + NO₂(g) → NO₂F (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. NO₂F (g) +F (g) Note: your answer should not contain the concentrations of any intermediates. rate constant rate = k 0+ 00 X Ś

The rate law for the reaction: NH4+ + NO₂ N₂ + 2H₂O is rate =k[NH4+][NO₂] It is found that the rate constant for this reaction is 3.05x10-4 M-1s-1. Calculate the rate of the reaction, including units, if [NH4*] is 0.265M and [NO₂] is 0.0803M. Attach File Browse Local Files