quickly please ### Chemistry Multiple-Choice Questions#### Question 25**If increasing the concentration of either reactant increases the overall rate of reaction, which is the most likely rate law for the reaction shown below?**\[ \text{CH}_{3}\text{CH}_{2}\text{Br}(\text{aq}) + \text{OH}^- (\text{aq}) \rightarrow \text{CH}_{3}\text{CH}_{2}\text{OH} (\text{aq}) + \text{Br}^- (\text{aq}) \]A) Rate = \( k[\text{CH}_{3}\text{CH}_{2}\text{Br}][\text{OH}^-]\)B) Rate = \( k[\text{CH}_{3}\text{CH}_{2}\text{Br}]^2 [\text{OH}^-]\)C) Rate = \( k[\text{CH}_{3}\text{Br}][\text{OH}^-]^2\)D) Rate = \( k[\text{CH}_{3}\text{CH}_{2}\text{OH}] [\text{Br}^-]\)### Question 26**Why can the initial rate of reaction (the rate of the reaction during the time when the reaction first takes place) be used to determine the rate law of a reaction?**A) At the beginning of the reaction, the reactants are at their highest concentration and monitoring the rate of the reaction when initial concentrations are changed provides information about how each reactant impacts the rate.B) At the beginning of the reaction, the reaction is at its slowest point, and therefore this provides information about how the reactants are interacting with each other in the reaction.C) At the beginning of the reaction, the reactants behave as catalysts and can lower the activation energy of the reaction.D) All of the above.E) A, B, and C are correct.#### Question 28**The decomposition of hydrogen peroxide is shown below. If the first order time-integrated rate constant for this reaction is 3.21 x 10^5 sec^-1, how long will it take for half of the initial hydrogen peroxide to decompose?**\[ 2\text{H}_2\text{O}_2(l) \rightarrow 2\text{H}_2\text{O}(l) + \text{O}_

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25. If increasing the concentration of either reactant increases the overall rate of reaction, which is the most likely rate law for the reaction shown below? CH₂CH₂Br(aq) + OH-(aq) → CH3CH₂OH(aq) + Br(aq) A) Rate = k[CH₂CH₂Br] [OH-] B) Rate = k[CH3CH₂Br][ OH-]0 C) Rate = k[CH3CH₂Br][OH-] D) Rate = K[CH3CH₂OH] [Br] E) Rate k[CH3CH₂OH][Br] =

25. If increasing the concentration of either reactant increases the overall rate of reaction, which is the most likely rate law for the reaction shown below? CH₂CH₂Br(aq) + OH-(aq) → CH3CH₂OH(aq) + Br(aq) A) Rate = k[CH₂CH₂Br] [OH-] B) Rate = k[CH3CH₂Br][ OH-]0 C) Rate = k[CH3CH₂Br][OH-] D) Rate = K[CH3CH₂OH] [Br] E) Rate k[CH3CH₂OH][Br] =

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 110CP: Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s)...

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(a) From data in Table 11.1, calculate the rate of reaction for each time interval: (i) from 40.0 s to 60.0 s; (ii) from 20.0 s to 80.0 s; (iii) from 0.0 to 100.0 s. (b) Use all of the data in the first two columns of Table 11.1 to draw a graph with time on the horizontal (x) axis and concentration on the vertical (y) axis. Draw a smooth curve through the data. On the graph, draw lines that correspond to [Cv+]/t for each interval. (c) Why is the rate not the same for each time interval in part (a), even though the average time for each interval is 50.0 s? (That is, for interval i, the average time is (40.0 s + 60.0 s)/2 = 50.0 s.) Write an explanation of the reason for a friend who is taking this course, and ask your friend to evaluate what you have written.
Compare the functions of homogeneous and heterogeneous catalysts.
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
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).
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.
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?
Why awe elementary reactions involving three or more reactants very uncommon?
Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
Given the following reactions and the corresponding rate laws, in which of the reactions might the elementary reaction and the overall reaction be the same? (a) Cl2+COCI2COrate=k[ CI2]3/2[CO] (b) PCI3+CI2PCI5rate=k[PCI3][CI2] (c) 2NO+H2N2+H2Orate=k[NO][H2] (d) 2NO+O22NO2rate=k[NO]2[O2] (e) NO+O3NO2+O2rate=k[NO][O3]
Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) 2 HI(g)Rate = k[H2][I2] Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. (a) The reaction must occur in a single step. (b) This is a second-order reaction overall. (c) Raising the temperature will cause the value of k to decrease. (d) Raising the temperature lowers the activation energy for this reaction. (e) If the concentrations of both reactants are doubled, the rate will double. (f) Adding a catalyst in the reaction will cause the initial rate to increase.
Ammonia decomposes when heated according to the equation NH3(g) NH2(g) + H(g) The data in the table for this reaction were collected at a high temperature. Plot In [NH3] versus time and 1/[NH3] versus time. What is the order of this reaction with respect to NH3? Find the rate constant for the reaction from the slope.