Be sure to answer all parts. The rate law for the reaction NH, (aq) + NO, (aq) N2g) + 2H,0() is given by rate = k NH,NO, . At a certain temperature, the rate constant is 5.10 x 10 M's. Calculate the rate of the reaction at that temperature if NH,=0.321 M and NO,=0.150 M. %3D x 10 Mis Enter your answer in scientific notation.

Be sure to answer all parts. The rate law for the reaction NH, (aq) + NO, (aq) N2g) + 2H,0() is given by rate = k NH,NO, . At a certain temperature, the rate constant is 5.10 x 10 M's. Calculate the rate of the reaction at that temperature if NH,=0.321 M and NO,=0.150 M. %3D x 10 Mis Enter your answer in scientific notation.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.99QE

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The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
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