Nitric oxide reacts with hydrogen at a measurable rate at 1000 K according to the following equation: 2NO + 2H2→ N2+ 2H2O The experimental rate law is Rate = k[NO]?[H2]. If time is measured in minutes and concentration is measured in moles per liter, what are the units for the rate of consumption of hydrogen? O ?'{mol2- min). mol/(L2. min). mol?/(L2. min). mol/(L3. min). mol/(L · min). O O O O

Nitric oxide reacts with hydrogen at a measurable rate at 1000 K according to the following equation: 2NO + 2H2→ N2+ 2H2O The experimental rate law is Rate = k[NO]?[H2]. If time is measured in minutes and concentration is measured in moles per liter, what are the units for the rate of consumption of hydrogen? O ?'{mol2- min). mol/(L2. min). mol?/(L2. min). mol/(L3. min). mol/(L · min). O O O O

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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2H2O2(aq) --> 2H2O(l) + O2(g) rate expression: rate = k[H2O2]m[I-]n 1. a) What experimental factors change the numerical value of n in the rate law for the reaction of H2O2 with I-? b) What experimental factors change the numerical value of k in the rate law for the reaction of H2O2 with I-?
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