Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction rate constant 1 NO₂(g) - NO(g) + O(g) k₁ 2 O(g) + NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₁»k₂. That is, the first step is much faster than the second. Write the balanced 0 chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K2, and (if necessary) the rate for Check constants l Explanation rate = k k =

2) Use the data below to determine the rate law and the value of k for the following reaction H2O2 (aq) + 3 I (aq) + 2H* (aq) →13° (aq) + H20 (1) Experiment [H20z] (M) [F] (M) [H*] (M) Initial Rate 0.0390 0.0470 0.0309 5.149 x 10-6 0.0779 0.0470 0.0309 1.030 x 10-5 2.059 x 10-5 5.149 x 10-6 3 0.0390 0.0939 0.0309 4 0.0390 0.0470 0.0620

Solve all three parts otherwise I will downvote...

Determine the rate law for the formation of oxygen predicted by this mechanism. (Assume the steady-state approximation is valid for any reaction intermediates.) k₁ CIO + CIO + M (CIO)₂ → CIOO + Cl (CIO)2 + sunlight k3 C100 + M k4 →→ Cl + O₂ 2x (C1 + 03 net: 2 033 0₂ → CIO + O₂) (this reaction occurs twice in the mechanism)

(a) In the reaction mechanisms given, there are some chemical species which will get produced in one step and get consumed in the other step and that are not in reactants nor in products of the total reaction. Such species are known as intermediates of a reaction as the name suggests. Therefore, in mechanism 1, the intermediates are (CH3)2CHOH2+, Cl-, (CH3)2CH+. and in mechanism 2: (CH3)2CHOH2+, Cl-. These ions are neither reactants nor products of the given total equation.

d) The integrated rate law for a reaction, describes how the reaction rate depends on the concentration of reactants. True False

Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant (g) (g) (g) (g) (g) (g) Suppose also ≫. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism.

Consider this reaction: 2H₂PO4 (aq) → P₂O5 (aq) + 3H₂O (aq) At a certain temperature it obeys this rate law. rate = (0.069 M¹.¹) [H₂PO4] Suppose a vessel contains H₂PO4 at a concentration of 0.380 M. Calculate how long it takes for the concentration of H3PO4 to decrease to 5.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. ? Submit A Continue 2 X

Determine the rate law for the reaction, 2IC1 + H2 = I, + 2HCi, from the following initial rate data: Initial Rate(Ms') 2.04x102 4.08x102 2.55x103 5.09x103 [H,], [ICI], 0.250 0.500 0.500 0.500 0.125 0.125 0.125 0.250 A) R = k[IC1]? В) R = k[H2]? C) R = k[ICI][H_]? D) R = k[ICl][H,] E) R = k[ICI]°[H¿] 000

For the gas phase decomposition of ethyl acetate, CH;COOC,H5–CH;COOH + C,H4 the rate constant in s1 has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.41×10“ K and a y-intercept of 28.8. The value of the rate constant for the gas phase decomposition of ethyl s1. acetate at 675 K is (Enter your answer to one significant figure.)