The reactionNO(g) + 02(g) – NO2(g) + O(g)plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series ofexperiments measured the rate of this reaction at a certain temperature and produced the following data:[02](mol L1)[NO]RateExpt(mol L)(mol L1s)10.00200.00505.0 x 101720.00200.0101.0 x 10160.00600.00501.5 x 1016A rate = k[NO]°[O2]?B rate = k[NO][O2]?Crate = k[NO]?[02]D) rate = k[NO][02]3. JUST A REMINDER, TAKE NOTEIN SOLVINGSummary of molecularity of elementary reactionsType of Elementary ReactionMolecularityRate LawA→ productsUnimolecularRate = k[A]%3DA + B → products2 A→productsRatek[A][B]%3DBimolecularRate = k[A]²%3DA + B + C → products2 A + B → productsRate = k[A][B][C]%3DTermolecularRate = k[A]°[B]A + B + C + D→ productsThe Arrhenius equation describes the temperaturedependence of the rate constant, k.Not observedEak = Ae RT- E, is the activation energy- R is the universal gas law constant• Ris 8.314 J mol K- T is the absolute temperature,- A is the proportionality constant called the frequency factor or0.693t1/2 =kpreexponential factor.

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Answered: rate of this reaction

Science

Chemistry

rate of this reaction

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.36PAE: The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in...

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