O KINETICS AND EQUILIBRIUM三Deducing a rate law from the change in concentration over timeA chemistry graduate student is studying the rate of this reaction:NH,OH (aq) → NH, (aq)+H,0 (aq)She fills a reaction vessel with NH,OH and measures its concentration as the reaction proceeds:time[NH,OH](milliseconds)0.500 M10.0.314 M20.0.197 M30.0.123 M40.0.0775 MUse this data to answer the following questions.Writo the rato lau fonr thir roationato - OExplanationCheckO 2021 McGraw-Hill Education. All Rights ReservedTermsType here to search 20.0.197 M30.0.123 M40.0.0775 MUse this data to answer the following questions.Write the rate law for this reaction,rate = k|Calculate the value of the rate constant k.k = |Round your answer to 2 significant digits. Also besure your answer has the correct unit symbol.ExplanationCheckO 2021 McGraw-Hill Education. All Rights ReseO Type here to searchCbp

A set of data for the determination of rate constant, which is to be accomplished.

A chemistry graduate student is studying the rate of this reaction: NH,OH (aq) - NH, (aq)+H,0 (aq) She fills a reaction vessel with NH,OH and measures its concentration as the reaction proceeds: time [NH,OH] (milliseconds) 0.500 M 10. 0.314 M 20. 0.197 M 30. 0.123 M 40. 0.0775 M Use this data to answer the following questions. 0.

A chemistry graduate student is studying the rate of this reaction: NH,OH (aq) - NH, (aq)+H,0 (aq) She fills a reaction vessel with NH,OH and measures its concentration as the reaction proceeds: time [NH,OH] (milliseconds) 0.500 M 10. 0.314 M 20. 0.197 M 30. 0.123 M 40. 0.0775 M Use this data to answer the following questions. 0.

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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
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.
. Account for the increase in reaction rate brought about by a catalyst.
Isomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph. (a) What is the rate law for this reaction? (b) What is the equation for the straight line in this graph? (c) Calculate the rate constant for this reaction. (d) How long does it take for half of the sample to isomerize? (e) What is the concentration of CH3NC after 1.0 104 s?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
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?
At 40C, H2O2 (aq) will decompose according to the following reaction: 2H2O2(aq)2H2O(l)+O2(g) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2O2](mol/L) 0 1.000 2.16 104 0.500 4.32 104 0.250 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.16 104 s. Use this rate to calculate the average rate of production of O2(g) over the same time period. b. What are these rates for the time period 2.16 104 s to 4.32 104 s?