Answer all parts Use the following technique and the data below to verifythat the decomposition of nitrogen dioxide is second order.2NO₂(g) → 2NO(g) + O2(g)The rate law for the decomposition of nitrogen dioxide canbe written asRate = k[NO₂]", or k=whenn is the order of the reaction. Note that when you divide therates at various times by the concentrations raised to thecorrect powern, you should get the same number (the rate constantk). Divide each average rate in a time interval by the squareof the average concentration in that interval. Note that eachcalculation gives nearly the same value. Take the average ofthese calculated values to obtain the rate constant.Time0.00 min1.00 min2.00 min3.00 mink₁ =/(M.s)k₂ =/(M.s)k3 =/(M.s)Kaverage =/(M.s)[NO₂]0.3650 M0.3370 M0.3126 Mrate[NO₂]"0.2935 M Nitrogen monoxide reacts with oxygen gas to form nitrogen dioxide.2 NO(g) + O₂(g) → 2 NO₂(g)Determine the rate law for the following mechanism.Step 1, Fast equilibrium NO(g) + O₂(g) → OONO(g)Step 2, SlowNO(g) + OONO(g) → 2 NO₂(g)Rate =

Given Data: Time (min) [NO2] 0.00 min 0.3650 M 1.00 min 0.3370 M 2.00 min 0.3126 M 3.00…

Answered: Use the following technique and the…

Use the following technique and the data below to verify that the decomposition of nitrogen dioxide is second order. 2NO2(g) → 2NO(g) + O2(g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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