You perform a series of experiments for the reactionA----->B + C and find that the rate law has the formrate = k[A]x. Determine the value of x in each of the followingcases: (a) There is no rate change when [A]0 is tripled.(b) The rate increases by a factor of 9 when [A]0 is tripled.(c) When [A]0 is doubled, the rate increases by a factor of 8.

7.) The results of kinetics experiments have shown the rate of the following reaction:A + 2B + C ↓ products has the following rate law: rate = k[A]2[B]0[C]1with a rate constant of k = 1.3 × 10–4 L2/mole2·s (M –2·s–1).a.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 0.3, and 0.4 M, respectively?b.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 2.7, and 0.4 M, respectively?

Consider the reaction below at 100oC  T2U (g)  ⟶⟶ 2 T (g)  + U (g)  When [T2U] = 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U]o = 0.144 M, the reaction rate is 3.09 x 10-3 M/s, which is the numerical value of the specific-rate constant, k, for this reaction?  A. 0.149 B. 0.0372 C. 0.0667 D. 0.250

The differential rate laws for the balanced chemical reaction: aA(aq) + bB (aq) + CC (aq) → product is given by: raterxn = k [A]³[C]³ [B]³ What are the order in each chemical, as well as the overall order of the chemical kinetics? Place your answer in each box, respectively! Provide detailed solution (The order of kinetics in A) = (The order of kinetics in B) = (The order of kinetics in C) = (The overall order of kinetics) =

5.) For the reaction X + Y ↓ Z; the reaction rate is found to depend only upon the concentration of X. A plot of 1/[X] verses time gives a straight line. What is the rate law for this reaction?

4. The rate law for the reaction H₂ (g) + I₂ (g) → 2 HI (g) was determined to be rate = k [H₂] [1₂], which led to a simple single-step bimolecular mechanism where an H₂ molecule simply collided with an I₂ molecule. In the 1960s, though, different teams found spectroscopic evidence for this mechanism: (1) (2) (3) I₂ (g) →21 (g) H₂(g) + I (g) → H₂I (g) H₂I (g) + I (g) → 2 HI (g) (fast) (fast) (slow) Show that this mechanism is consistent with the rate law: rate = k [H₂] [1₂]. To do this, assign individual rate constants for ALL forward and reverse reactions in the mechanism (I'm guessing k₁, k-1, k2, k-2 and k3). Then show that the overall rate law from combining individual rate laws for the mechanism steps yields rate = (some combination of k's) [H₂] [1₂], and thus k= (some combination of k's). Remember that there should be no reaction intermediates in the rate law, only reactants. \

Consider the following balanced chemical equation: H2O2 (aq) + 3 r (aq) + 2 H (aq) >l (aq) + 2 H,O (I) If the concentration of iodide (la) decreases from 0.718 M to 0.426 M in the first 15 seconds, what is the rate of reaction? (A) (B) (C) (D) (E) 0.0195 M/s 0.292 M/s -0.00195 M/s 0.00649 M/s 0.0973 M/s

Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. Reaction (a) C₂H5CI → C₂H4 + HCI (b) HO + NO₂ + Ar → HNO3 + Ar (c) O + H₂S →→→→HO + HS Molecularity. Rate expression rate = rate = rate

Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. Reaction Molecularity Rate expression (a) NO2 + NO2→2 NO + 02 rate = (b) BrONO- ЭBro + NOz rate = (c) 0+ 02 + M 03 + M rate = unimolecular bimolecular termolecular

Assume that the formation of nitrogen dioxide, 2 NO(g) + 02(g) – 2 NO2(g) is an elementary reaction. (a) Write the rate law for this reaction. (Rate expressions take the general form: rate = k. [A]ª . [B]b.) chemPad О Help Greek - rate=k•[NO]2.[02] rate=k*[NO]^2*[O_2] Correct. (b) A sample of air at a certain temperature is contaminated with 1.9 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. If not, repeat your answer from above. (Rate expressions take the general form: rate = k . [A]ª . [B]b. Use k' for the new rate constant as needed.) chemPad O Help Greek - rate=k':[NO]2 rate=k*[NO]^2 Correct. (c) Under the conditions described in (b), the half-life of the reaction has been estimated to be 6.7x103 min. What would the half-life be if the initial concentration of NO were 12.4 ppm? 4.0 |1030192 X min Supporting Materials Periodic Table Constants and E Supplemental Data