The reaction of butyl chloride with water is a first-order reaction. (a) Use the following graph to estimate the half-life of the reaction. (b) Calculate the rate constant. C4H,CI(aq) + H,0(1) →C4H,OH(aq) + HCI(aq) 0.100 Instantaneous 0.090 rate at t = 0 s (initial rate) 0.080 Instantaneous rate at 0.070 time t = slope of tangent to the line at 0.060 time t. 0.050 Instantaneous rate at t = 600 s 0.040 0.030 0.020 At 0.010 100 200 300 400 500 600 700 800 900 Time (s) [C,H9CI] (M) A [C¿H,CI]

Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. (a) O + H₂S Reaction HO + HS (b) OH + NO2 + N₂ HNO3 + N2 (c) CH3CHO → CH3 + CHO Molecularity. ][ Rate expression rate = rate = rate =

17) For the following reaction give the expression for the average rate for each species in the equation. 3 Ag₂S(s) + Al(s) + 3 H₂O(1)→6 Ag(s) + Al₂O3(s) + 3 H₂S(aq)

Cyclopropane isomerizes to propylene according to a first- order reaction: cyclopropane → propylene The activation energy is E, = 272 kJ mol-1. At 500°C, the reaction rate constant is 6.1 × 10-4 s-1. (a) Calculate the Arrhenius factor A for this reaction. (b) Calculate the rate constant for this reaction at 25°C.

Be sure to answer all parts.The reaction2A → Bis second order in A with a rate constant of 37.9 M−1 · s−1 at 25°C.(a) Starting with [A]0 = 0.00701 M, how long will it take for the concentration of A to drop to 0.00180 M?s(b) Calculate the half-life of the reaction for [A]0 = 0.00701 M.s(c) Calculate the half-life of the reaction for [A]0 = 0.00215 M.

Consider the following reaction: Q:4-1 2 NO(g) + 2 H;(g) → N;(8) + 2 H,0(g) (a) The rate law for this reaction is first order in H, and second order in NO. Write the rate law. (b) If the rate constant for this reaction at 1000 K is 6.0 × 10ª M-²s¯!, what is the re- action rate when [NO] = 0.035 M and [H,] = 0.015 M? (c) What is the reaction rate at 1000 K when the concentration of NO is increased to 0.10 M, while the concentration of H, is 0.010 M? (d) What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and [H,] is increased to 0.030 M? %3D

The reaction N2O5- 2NO2 + 1/2 O2(g) is first order. The rate constant k is 6.2 x 10-4/min. A) What is the half life of this reaction in seconds and days? B) How long will it take for the concentration of N2O5 to decrease to 25% of it's original concentration?

Experiments show that each of the following redox reac-tions is second order overall:Reaction 1: NO₂(g)+CO(g) →NO(g)+CO₂(g) Reaction 2: NO(g)+O₃(g) →NO₂(g)+O₂(g) (a) When [NO₂] in reaction 1 is doubled, the rate quadruples.Write the rate law for this reaction.(b) When [NO] in reaction 2 is doubled, the rate doubles. Writethe rate law for this reaction.(c) In each reaction, the initial concentrations of the reactantsare equal. For each reaction, what is the ratio of the initial rateto the rate when the reaction is 50% complete?(d) In reaction 1, the initial [NO₂] is twice the initial [CO].What is the ratio of the initial rate to the rate at 50% completion?(e) In reaction 2, the initial [NO] is twice the initial [O₃]. Whatis the ratio of the initial rate to the rate at 50% completion?

Be sure to answer all parts. The reaction 2A → B is second order in A with a rate constant of 31.7 M−1 · s−1 at 25°C. (a) Starting with [A]0 = 0.00713 M, how long will it take for the concentration of A to drop to 0.00180 M?  (b) Calculate the half-life of the reaction for [A]0 = 0.00713 M.  (c) Calculate the half-life of the reaction for [A]0 = 0.00203 M.

[4] Consider the following mechanism for the reaction of nitric oxide and hydrogen: kı 2NO(g)+ H2(g) → N;O(g) + H¿O(g) slow k2 N,0(g) + H2(g) → N2(g) + H2O(g) fast (a) Write an equation for the overall reaction. (b) Write the theoretical rate law for the above mechanism. (c) Is a catalyst involved in the above mechanism? If so, what is it? (d) Are there any reaction intermediates? If so, list them.