3) Ozone and hydrazine,N.H, react to form water and nitrogen gas, If the rate of production of water is 2.0x10 H.O M/'s 2 Oslg)+SNg My (g)→6H20(4)+3N2G) a) What would the rate of the reaction be based on ozone? b) What woald the rate of the reaction be based on hydrazine? c) What would the rate of the reaction be based on nitrogen gas?

3) Ozone and hydrazine,N.H, react to form water and nitrogen gas, If the rate of production of water is 2.0x10 H.O M/'s 2 Oslg)+SNg My (g)→6H20(4)+3N2G) a) What would the rate of the reaction be based on ozone? b) What woald the rate of the reaction be based on hydrazine? c) What would the rate of the reaction be based on nitrogen gas?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 90QAP

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Similar questions

Express the rate of the reaction 2N2O(g)2N2(g)+O2(g) in terms of (b) [ N2O ] (a) [ O2 ]
The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant. Rate [H2OJ [Kll (mL min-’) (mol L ’) (mol L ’) 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066
A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
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Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
How do the rate of a reaction and its rate constant differ?
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The hypothetical reaction, A + B —*C, has the rate law Rate = When [A] is doubled and [B] is held constant, the rate doubles. But the rate increases fourfold when [B] is doubled and [A] is held constant. What are the values of'x and y?
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