The reaction H3C-1 OHH3C-OH+r may go by either of the following mechanisms: I) H3C-1 H3C++r (slow) H3C++ OH ® H3C-OH (fast) or II) H3C-1+ OHH3C-OH+I* If the first mechanism were correct, what would be the rate law? Rate = K[H3C-1] Rate = K[H3C-1][OH] Rate = k[H3C-1][OH-]2 Rate = K[H3C][OH] Rate = K[H3C+]

The reaction, NO₂Cl(g) + CI(g) -> NO2(g) + Cl₂(g), was found to be first order in each of the two reactants and second order overall. The rate law is therefore rate = k[NO₂]² rate = k[NO₂][ Cl₂] rate = k[CI] rate = K[NO₂CI][CI][NO₂][C1₂] rate = K[NO₂CI][CI]

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

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Order and rate law of a reaction The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is rate = k[NO₂)² The exponent "2" is used because the reaction involves two NO₂ molecules. The rate law for step 2 is because the reaction involves only one molecule of each reactant the exponents are omitted. Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1.2A B+C 2. B+D+E+C Part A What is the overall reaction? Express your answer as a chemical equation. ► View Available Hint(s) for Part A for Pardo for Part redo foPart A refor Part A keyboard shortcuts for Part A help for Part A A chemical reaction does not occur for this question. Submit Part B Which species is a reaction…

For the reaction            H2(g) + C2H4(g) ⟶⟶C2H6(g) A series of experiments were conducted as sown in the Table.  If the rate law were found to be :           rate = k[H2][C2H4] what is the missing initial rate (marked with a "?" in the Table)?

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Consider the following reaction: 12 (g) + H2 (g) --> 2 HI (g). Given the mechanism below, determine the rate law for the equation. Note: input the rate law following the format rate-k[A]2[B2] with no spaces don't worry about formatting upper or lower case. 1₂ (g) 21 (g) (fast) H₂ (9)+21 (g) → 2HI (g) (slow)