Section 5. For a different reaction, the plot of the natural log of concentration versus time in seconds plot was linear with a slope of -0.156 s¹. a. What is the order of this reaction? 1st order b. What is the rate law of this reaction? C. What is the integrated rate law of this reaction? d. Calculate the rate of the reaction if the concentration is 0.35 M. Show your work. Date

Section 5. For a different reaction, the plot of the natural log of concentration versus time in seconds plot was linear with a slope of -0.156 s¹. a. What is the order of this reaction? 1st order b. What is the rate law of this reaction? C. What is the integrated rate law of this reaction? d. Calculate the rate of the reaction if the concentration is 0.35 M. Show your work. Date

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

5. For the reaction below, initially 3-5 mol of NH, are placed in a 4.0 L reaction chamber. After 3.0 minutes only 1.6 moles of NH, remain. SHOW ALL YOUR WORK. 4 NH,(g) + 50,(g)-4 NO(g) + 6 H,0(g) a. Calculate the average rate of reaction with respect to NH,. b. Calculate the average rate at which H,0 is being formed. c. Calculate the average rate at which O, is being consumed. (answer + units for NH) (answer + units for H,0) (answer + units for O)
The rate law for the reaction A + 3B → C + 2D was found to be v=kr[A][B]^2 .a. What are the units of kr when the concentrations are in moles per cubic decimeter and the time is in seconds. b. Express the rate law in terms of the rates of consumption of A. c. Express the rate law in terms of the rate of formation of D.
6. The rate law for the overall reaction 2 N2O5 (g) →4 NO2 (g) + O2 (g) is Rate = k[N2O5). a. Consider this mechanism: i. N2O5 (g) → NO: (g) + NO2 (g) ii. NO2 (g) + N2Os (g) →3 NO2 (g) + O2 (g) i. NO: (g) +0 (g) → NO2 (g) + O2 (g) Is this reaction mechanism consistent with the rate law? Why or Why not? [fast) [slow] [fast] b. If the reacuion mechanism is not consistent with the rate law, how would it need to change to become consistent? c. List potential reaction intermediates present in uNIS nechanism d. Draw a reaction energy diagram for this mechanism including any modifications you've made in a-c.
A particular reaction is proposed to be first order. What plot would support this conclusion? a. a linear plot of [reactant] versus time b. an exponential decay of [reactant] versus time c. a linear plot of ln [reactant] versus time d. an exponential decay of ln [reactant] versus time
At 330 degrees Celsius, the rate constant for the second order decomposition of NO2 is 0.775M ^ - 1 * s ^ - 1 the Initial concentration of NO2 is 0.0500M a. Write the rate law expression for this reaction b. What is the concentration of NO2 after 30.0 minutes? c. How long in minutes will it take the concentration to decrease to 0.0050M? d. What is the half life for this reaction? e. What effect would doubling the NO2 concentration have on the rate of the reaction?
14
A chemistry graduate student is studying the rate of this reaction: NH4OH(aq)—>NH3(aq)+H2O(aq) He fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds (shown in picture). A. Write the rate law for this reaction B. Calculate the value of the rate constant k. Round your answer to two significant digits. Also be sure your answer has the correct unit symbol.
36 The reaction C2H5Cl →C2H4 + HCl is first order in C2H5Cl. The rate constant is 1.60 x 10-6/s. In an investigation of the decomposition of C2H5Cl an initial concentration of 0.165 mol/L was used. What will the concentration of C2H5Cl be after 125 hours? Select one: a. 0.0803 M b. 0.0703 M c. 0.0603 M d. 0.0503M
B 8. D Trial 1 2 3 4 [A₂] 0.10 0.20 0.30 0.30 [B] 0.50 0.50 0.05 0.10 An experiment was conducted to determine the rate law for the reaction A2(g) + B(9) A₂B(g). The table above shows the data collected. Based on the data in the table. which statement is correct? Initial rate (Ms-¹) 2.5 x 10 5.0 x 10-4 5.0 × 10-5 1.0 x 10-4 Since the rate law can be expressed as ratek[A₂), tripling the concentration of A2 will cause a 9-fold increase in the rate of the reaction. Since the rate law can be expressed as rate k[A₂][B], doubling the concentrations of A₂ and B will quadruple the rate of the reaction. Since the rate law can be expressed as rate k[A] [B], tripling the concentration of A2 while keeping the concentration of B constant will triple the rate of the reaction. Since the rate law can be expressed as rate=k[A₂][B], doubling the concentration of B while keeping the concentration of A₂ constant will double the rate of the reaction.
16 The reaction C2H5Cl →C2H4 + HCl is first order in C2H5Cl. The rate constant is 1.60 x 10-6/s. In an investigation of the decomposition of C2H5Cl an initial concentration of 0.165 mol/L was used. How many hours will it take for 75% of C2H5Cl to decompose? Select one: a. 241 b. 341 h c. 541 d. 841
The reaction between hydrogen and chlorine is as follows: Cl2(g) + H2(g) → 2HCl(g) Experiments show that this reaction is first order with respect to H2 and one-half order with respect to Cl2. What is the rate law? a. Rate = k [H2]1/2 [Cl2] b. Rate = k [Cl2] [H2]2 c. Rate = k [Cl2]1/2 [H2] d. Rate = k [Cl2]2 [H2]
For the reaction below, a series of experiments was conducted and the data collected in the table below. a. Determine the rate law and the overall order of the reaction. b. Calculate the rate constant, including appropriate units. c. Determine the initial rate when the initial concentrations of both reactants are 0.12 M. Reaction (might be unbalanced): NO (g) + Cl2 (g) → NOCI (g) Experiment Data: Experiment # Initial [NO] (M) Initial [Cl2] (M) Initial Rate (M/s) 0.13 1.0x10-2 0.20 2 0.26 0.20 4.0x10-2 3 5.0x10-3 0.13 0.10