None a) On a single graph, sketch [A], [X], and [Y] as a function of time for the reaction A→X+2Y. Usethe following initial concentrations: [A]0 = 0.50 M and [X] = [Y]=0.What are the concentrations of A, X, and Y after completion of the reaction?

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Answered: a) On a single graph, sketch [A], [X],…

Chemistry

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Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 63AE: For the following reaction profile, indicate a. the positions of reactants and products. b. the...

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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.
For the following reaction profile, indicate a. the positions of reactants and products. b. the activation energy. c. E for the reaction.
Give at least two physical properties that might be used to determine the rate of a reaction.
Consider the decomposition reaction 2X2Y+ZThe following graph shows the change in concentration with respect to time for the reaction. What does each of the curves labeled 1, 2, and 3 represent?
How do chemists envision reactions taking place in terms of the collision model for reactions? Give an example of a simple reaction and how you might envision the reaction’s taking place by means of a collision between the molecules.
You carry out the following reaction by introducing N2O4 into an evacuated flask and observing the concentration change of the product over time. N2O4(g)2NO2(g) Which one of the curves shown here reflects the data collected for this reaction?
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?
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.
(Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a 10-K rise in temperature increases the reaction rate by two to four times. Use an average increase of three times to answer the questions below. (a) What is the approximate activation energy of a typical chemical reaction at 298 K? (b) If a catalyst increases a chemical reactions rate by providing a mechanism that has a lower activation energy, then what change do you expect a 10-K increase in temperature to make in the rate of a reaction whose uncatalyzed activation energy of 75 kJ/mol has been lowered to one half this value (at 298 K) by addition of a catalyst?

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a) On a single graph, sketch [A], [X], and [Y] as a function of time for the reaction A→X+2Y. Use the following initial concentrations: [A]0 = 0.50 M and [X] = [Y]=0. What are the concentrations of A, X, and Y after completion of the reaction?