Ammonia can react with oxygen to produce nitric oxide and water.4NH3(g) + 502(g) → 4NO(g) + 6H2OThe rate at which ammonia is consumed in a laboratory experiment is 4.06 mol/L s. At what rate is watervapor produced?Round your answer to 2 decimal places. 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 K1- T is the absolute temperature,- A is the proportionality constant called the frequency factor or0.693t1/2 =kpreexponential factor.

For the balanced chemical reaction, The rate of reaction is (-1/4)□[NH3]/□t = (1/6)□[H2O]/□t So,…

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Chemistry

at which ammonia is consumed in a laboratory experiment is 4.06 oduced? our answer to 2 decimal places.

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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