(a) For a reaction, A + B > Product, the rate law is given by,Rate = k [A]1 [B]2 . What is the order of reaction?(b) Write the unit of rate constat ‘k’ for the first order reaction.

The decomposition of XY is second order in XY and has a rate constant of 7.41 × 10−3 L·mol−1·s−1 at a certain temperature, the half-life for this reaction at an initial concentration of 0.101 mol·L−1 1336. A) If the initial concentration of XY is 0.225 mol·L−1, how long will it take for the concentration to decrease to 6.95 × 10−2 mol·L−1 ?, B) If the initial concentration of XY is 0.080 mol·L−1, what is the concentration of XY after 75 s ?

Be sure to answer all parts. The reaction between NO2 and CO to produce NO and CO2 is thought to occur in two steps: Step 1: NO2 + NO2     NO + NO3 Step 2: NO3 + CO     NO2 + CO2 The experimental rate law is rate = k[NO2]2. (a) Write the equation for the overall reaction. Do not include phase abbreviations.      (b) Identify the intermediate(s).     NO3    NO2    NO    CO2    CO (c) Identify the rate-determining step.     Step 1    Step 2    Neither step

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) =

a)A nickel catalyst is commonly used in the hydrogenation of ethylene. If the initial concentration of ethylene is 2.75 mol·L−1 and the rate constant for the reaction is 0.0018 mol·L−1·s−1, what is the rate of reaction if it follows a zero-order reaction mechanism? Express your answer to two significant figures. b)Determine the half-life for the reaction in Part B. Express your answer to two significant figures.

Consider the following reaction: 2A + B + 3C. (a) Write an expression for the overall rate; (b) What are the rates at which A and B are consumed and generated if C is created at a rate of 0.015 M/min?

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.

You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: (b) For a reaction of the form, A + B + C --> reaction from the choices below. (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A] [B]Y? Choose all correct possibilities. O [A] = 0.2 and [B] = 1.0 O [A] = 0.4 and [B] = 1.0 O [A] = 0.8 and [B] = 0.5 O [A] = 0.6 and [B] = 0.5 O [A] = 0.2 and [B] = 1.5 O [A] = 0.4 and [B] = 0.5 O [A] = 0.4 and [B] = 1.5 O [A] = 1.0 and [B] = 0.5 O Rate = K[A][B][C] O Rate = K[A][C] O Rate = K[A]²[C] T O Rate = k[A][C]² O Rate = K[A]²[C]² O Rate = K[A]³ [c] O Rate = K[A][C]³ the following Experiment [A] (M) [B] (M) Rate (M/s) 0.5 0.5 The rate will be the original rate multiplied by a factor of 0.2 0.4 (c) By what factor will the rate of the reaction described in part (b) above change if the…

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