Consider the following reaction:  H2+ 2 ICl → 2 HCl + I2 The experimentally determine rate law for this reaction is rate = k[H2][ICl]. Determine which mechanism is plausible. A)  ICl + ICl → I2 + Cl2    (1) slow      Cl2 + H2→ 2 HCl        (2) B) H2+ ICl → HI + HCl     (1) slow     ICl + HCl → HI + Cl2    (2) C) H2+ ICl → HCl + HI      (1) slow      HI + ICl → HCl + I2      (2)

Consider the following reaction: 2 CH3l (aq) C2H6 (g) + 12 (g) This reaction is first-order, and its rate constant, k at 25°C is 0.0115 s¹. a) If the initial concentration of CH3l is 6.75 M, what is the concentration of CH3I after the reaction has been carried out for 1.83 hours? Report your answer using most of the decimal places reported on your calculator. Do not use scientific notation [CH31]= M b) If the rate constant is increased by a factor of 2.36 when the temperature is raised from 25°C to 76.6 °C, what is the activation energy (in kJ/mol) for this reaction? Report your answer using most of the decimal places reported on your calculator. Do not use scientific notation Ea kJ/mol

The reaction 2 NO(9) + 02 (9) → 2 NO2(9) was studied, and the following data were obtained where A[02] Rate = At NOo [02]o Initial Rate (molecules/cm³) (molecules/cm) (molecules/cm° · s) 1.00 x 1018 1.00 x 1018 2.00 × 1016 3.00 x 1018 1.00 x 1018 1.80 x 1017 2.50 × 1018 2.50 × 1018 3.13 x 1017 What would be the initial rate for an experiment where [NO], = 2.66 × 1018 molecules/cm° and [O2]o 1.48 x 1018 molecules/cm°? Rate = |molecules/cm³ . •S

For the decomposition of gaseous dinitrogen pentaoxide,2N₂O₅(g) →4NO₂(g) +O₂(g), the rate constant is k=2.8X10⁻³ s⁻¹at 60°C. The initial concentration of N₂O₅ is1.58 mol/L. (a) What is [N₂O₅] after 5.00 min? (b) What frac-tion of the N₂O₅ has decomposed after 5.00 min?

The initial rate of the reaction is determined for different initial conditions, with the results listed in the table. (a) What is the overall reaction order? (b) What is the value of the rate constant, k

At a certain temperature the rate of this reaction is first order in C1₂O5 with a rate constant of 0.0699 s ! 2C1₂O5 (g) → 2Cl₂ (g) +50₂ (g) Suppose a vessel contains Cl₂05 at a concentration of 0.910M. Calculate the concentration of C1₂05 in the vessel 11.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś

Consider the following reaction: 1. 2 N,O5 (g) → 4 NO, (g) + O, (g) The initial concentration of N2O5 was 0.48 mol/L, and 25 minutes after initiating the reaction, all of the N,Os has been consumed. (a) Calculate the average rate of the reaction over this 25-minute time interval. (b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer.

One of the reactions that occurs in polluted air in urban areas is 2NO2(g) + O3(g) –→N2O5(g) + O2(g). Assume that a species with the formula NO3 is involved in the mechanism, and the observed rate law for the overall reaction is rate = k[NO2][O3]. Propose a mechanism for this reaction that includes the species NO3 and is consistent with the observed rate law. NO2(g) + O3(g) – NO3(g) + O2(g) (fast) NO3(g) + NO2(g) → N2O5(g) (slow) NO2(g) + O3(g) – NO3(g) + O2(g) (fast) 4NO3(g) 2N2O5(g) + O2(g) (slow) NO2(g) + O3(g) –→ NO3(g) + O2(g) (slow) NO3(g) + NO2(g) → N2O5(g) (fast) NO2(3) + O3(g) → NO3(g) + O2(g) (slow) 4NO3(3) → 2N20O5(g) + O2(g) (fast)

Consider the mechanism. Step 1: 2A — В +С slow Step 2: В +С — Е fast Overall: 2А — Е Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate =

9)  The following three-step mechanism has been proposed for the reaction of chlorine and chloroform.                                                                                    rate constants 1)   Cl2(g) ↔   2 Cl(g)                   Keq1 =2.5         k1 = 5.5 x 103  sec-1      2)   Cl(g) +   CHCl3(g)   →   HCl(g)   +   CCl3(g)   k2 = 2.4 x 10−2 M-1sec-1 3)   CCl3(g) +   Cl(g)   →   CCl4(g)                         k3 = 3.6 x 102 M-1sec-1   a)  Write the equation for the overall reaction. __a__   b)  Write the rate law for the overall reaction. __b__   c)  Calculate the rate constant for the overall reaction (include units) __c__