Explanation The given reaction between NO ( g ) and O 2 ( g ) is, 2 NO ( g ) + O 2 ( g ) → 2 NO 2 ( g ) The given information for this reaction is, From the experimental determination, the rate is second order in NO and first order in O 2 . The rate law for the given reaction is represented as, Rate = k [ NO ] 2 [ O 2 ] Where, k is the rate constant. [ NO ] is the concentration of NO . [ O 2 ] is the concentration of O 2 . 2 is the order of NO . The rate for the given mixtures can be determined by using the rate law by putting the values for the concentration of NO and O 2 in the rate law. In the given mixtures, the combination of a blue and a red sphere represents the NO molecule and the combination of two red spheres represents the O 2 molecule. In mixture ( 1 ) , there are five molecules of NO and four molecules of O 2

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ISBN: 9780134562230

Author: Brown

Publisher: PEARSON

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Chapter 14, Problem 5E

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To determine: The correct mixture of NO(g) and O2(g) that will have the fastest initial rate.

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Chapter 14, Problem 4E

Chapter 14, Problem 6E

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Chapter 14 Solutions

CHEMISTRY: THE CENTRAL SCIENCE

Ch. 14.2 - If the experiment in Figure 14.2 is run for 60 s,...Ch. 14.2 - Prob. 14.1.2PE Ch. 14.2 - Which of the following could be the instantaneous...Ch. 14.2 - Using Figure 14.3, determine the instantaneous...Ch. 14.2 - At a certain time in a reaction, substance A is...Ch. 14.2 - Prob. 14.3.2PE Ch. 14.3 - Suppose the rate law for the reaction in this...Ch. 14.3 - Assuming that rate = k[A][B], rank the mixtures...Ch. 14.3 - Prob. 14.5.1PE Ch. 14.3 - Prob. 14.5.2PE

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The correct mixture of NO ( g ) and O 2 ( g ) that will have the fastest initial rate.

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To determine: The correct mixture of NO(g) and O2(g) that will have the fastest initial rate.

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Chapter 14 Solutions