Predict the initial rate of reaction in experiment 4.13.126. An important reaction in the formation of photochenmicsmog is the reaction between ozone and NO:NO(g) + O3(g) → NO2(g) + O,(g) The reaction is first order in NO and O3. The rate constantof the reaction is 80 Ms at 25°C and 3000 M¯' s¯' at13.75°C.If this reaction were to occur in a single step, would therate law be consistent with the observed order of thereaction for NO and O3?h What is the value of the activation energy of thea.reaction?c. What is the rate of the reaction at 25°C when [NO] =3 X 10-6 M and [O3] = 5 x 10-9 M?%3D%3Dd. Predict the values of the rate constant at 10°C and 35°C.

The rate law will be consistent, even though the reaction occurs in single step. The order of the…

Answered: Predict the initial rate of reaction in…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter16: Reaction Rates

Section: Chapter Questions

Problem 6STP

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Give at least two physical properties that might be used to determine the rate of a reaction.
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
. Account for the increase in reaction rate brought about by a catalyst.
Iodomethane (CH3I) is a commonly used reagent in organic chemistry. When used properly, this reagent allows chemists to introduce methyl groups in many different useful applications. The chemical does pose a risk as a carcinogen, possibly owing to iodomethanes ability to react with portions of the DNA strand (if they were to come in contact). Consider the following hypothetical initial rates data: [DNA]0 ( mol/L) [CH3I]0 ( mol/L) Initial Rate (mol/Ls) 0.100 0.100 3.20 104 0.100 0.200 6.40 104 0.200 0.200 1.28 103 Which of the following could be a possible mechanism to explain the initial rate data? MechanismIDNA+CH3IDNACH3++IMechanismIICH3ICH3++ISlowDNA+CH3+DNACH3+Fast
The reaction for the Haber process, the industrial production of ammonia, is N2(g)+3H2(g)2NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 ×10-5 molL-1s-1. At what rate is nitrogen consumed? At what rate is hydrogen consumed?
Candle wax is a mixture of hydrocarbons. In the reaction of oxygen with candle w ax in Figure 11.2, the rate of consumption of oxygen decreased with time after the flask was covered, and eventually' the flame went out. From the perspective of the kinetic-molecular theory, describe what is happening in the flask. FIGURE 11.2 When a candle burns in a closed container, the flame will diminish and eventually go out. As the amount of oxygen present decreases, the rate of combustion will also decrease. Eventually, the rate of combustion is no longer sufficient to sustain the flame even though there is still some oxygen present in the vessel.
Express the rate of the reaction 2N2O(g)2N2(g)+O2(g) in terms of (b) [ N2O ] (a) [ O2 ]
The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
A rate of reaction depends on four variables (Question 13.1). Explain by means of an example how the rate law deals with each of these variables.
Nitrogen monoxide, NO, is believed to react with chlorine according to the following mechanism: NO+Cl2NOCl2(elementaryreaction)NOCl22NOCl(elementaryreaction) Identify any reaction intermediate. What is the overall equation?

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