Determine the initial rate in mole/L-min if the rate constant for a certain first-order reaction is 0.40/min and the initial concentration of the compound involved is 0.50 mol/L? 0.25 mole/L·min 0.50 mole/L-min 0.20 mole/Lmin 0.40 mole/L min Question 5 of 2 A Moving to the next question prevents changes to this answer. 58°F Sunny End Fn 近

Determine the initial rate in mole/L-min if the rate constant for a certain first-order reaction is 0.40/min and the initial concentration of the compound involved is 0.50 mol/L? 0.25 mole/L·min 0.50 mole/L-min 0.20 mole/Lmin 0.40 mole/L min Question 5 of 2 A Moving to the next question prevents changes to this answer. 58°F Sunny End Fn 近

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...

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2) 2 NO₂ (g) +2 NO(g) + O₂(g) (W) [ZON] 2.5 2 1.5 1 0.5 0 10 20 Reaction Data 30 40 50 60 70 Time (s) 80 Use the experimental data for the above reaction to answer. a) What is the average rate of reaction between 50 and 70 seconds? b) Estimate the instantaneous rate of reaction at 20 seconds. 90 100 c) Estimate the instantaneous rate of formation of O₂ at 30 seconds. d) If the initial concentration of NO₂ is 2.0M how much O₂ is produced in the first 40 seconds of reaction?
The following results were obtained for the below reaction in experiments designed for the study of the rate of the reaction. A + B=> 2C Experiment Initial concentrations mol/L [A] [B] Rate of disappearance of A (M/sec) 1 0.030 0.030 2.0x10-3 2 0.030 0.060 4.0x10-3 4 0.060 0.030 4.0x10-3 Write the differential rate law for this reaction. What will be the initial rate of disappearance of A, if an experiment is attempted with A and B both equal to 0.060M? Write the integrated rate law for the concentration of A. Calculate the half-life for A Calculate the concentration of A in experiment 2 after 60 seconds rate constant = 2.22M^-1sec^-1
▼ Part A Consider the reaction Using the information in the following table, calculate the average rate of formation of P₂O, between 10.0 and 40.0 s. Time (s) 0 10.0 20.0 30.0 50.0 40.0 [P₂05] (M) 02.10×103 5.10×10-3 6.90×103 8.10×10-3³ 8.70x103 Express your answer with the appropriate units. ▸ View Available Hint(s) Submit Previous Answers Rate of formation of P₂O5 = 2.00-10-4 Part B Complete previous part(s) Part C ■ Consider the reaction x² * Incorrect; Try Again; 5 attempts remaining Enter your answer with a different unit type. Review a list of acceptable units HÅ Submit Previous Answers O x"² 5Br (aq) + Bro, (aq) + 6H+ (aq) →3Br₂(aq) + 3H₂O(1) The average rate of consumption of Bris 1.06x104 M/s over the first two minutes. What is the average rate of formation of Brg during the same time interval? Express your answer with the appropriate units. ▸ View Available Hint(s) ||||A HÅ Rate of formation of Br₂ = 7.04.10 5 . Ms-1 * Incorrect; Try Again; 5 attempts remaining x 10" M x 10"…
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67) A reaction is carried out in a container. A pure compound X is shown at the start of the experiment. Compound X undergoes a first order reaction to form compound Y, with no reverse reaction. Which of the following might represent the container at 20 minutes ? The diagram shows the number of molecules of each sample X and Y. t=0 mins 1-10 mins X 15 X=30 Y=0 Y = 15 t = 20 mins X = 15 Y = 15 Thaum Whic A) X = 7 Y = 23 C) D) X = 23 Y = 7 X = 0 Y = 30
1. The rate of the homogeneous gas-phase reaction: A + 3B → 2X + Y has been studied. Some of the data are: Initial total pressure change rate (-dP/dt) / (torr/s) Initial pressure A P/ torr 352 289 Initial pressure B P/ torr Run 153 392 3.44 6.55 8.14 3 4 247 617 (a) What are the orders of the reaction with respect to A and with respect to B? (b) Assume that the gas mixture is ideal and find the relation between the usual rate of reaction, v, and dP/dt, where P is the total pressure. The volume is constant.
consider the rate data at a certain temp for the reaction 2NO(g) + 2H2(g) --> N2(g) + 2H2O(g) determine the order of the reaction with respect to nitrogen monoxide
Use the data presented in the table to determine the rate equation for the hypothetical reaction shown. A(g) + 2B(g) + 3C(g) [Math Processing Error] D(g) + 2F(g) Exp {A} (M) {B} (M) {C} (M) initial rate (M/min) 0.0025 0.0025 0.0025 3.16x10-11 0.0025 0.0050 0.0025 1.27x10-10 3 0.0050 0.0050 0.0025 1.27x10-10 4 0.0100 0.0100 0.0050 4.06x10-9 What is the reaction order with respect to A? What is the reaction order with respect to B? What is the reaction order with respect to C? Enter each of your answers numerically as integers or fractions (ex: 0, 1/2, 1, 3/2, 2, 3, etc). Hint: Determining the order of one of the reactants will be difficult. Determine the order of the two easy reactants first, then use that information in determining the difficult one.
The following set of data was obtained for the reaction below. What is the rate of reaction when [NO] = 0.00105M and [H2] = 0.0083M? . 2H2(8) + 2NO(8) 2H2O(g) + N2(8) Exp [NO], M [H2]. M Rate, M/s 1 0.0060 0.0010 0.180 2 0.0060 0.0020 0.360 3 0.0010 0.0060 0.030 4 0.0020 0.0060 0.120 5.0 x 106 Ms-1 43.5 Ms-1 -1 0.046 Ms 1.3 x 10-4 Ms-1
The decomposition of O, is a second order reaction with a rate 3 constant of 50.5 M hr-¹. 2 O3(g) → 3 02 (9) What is the half-life for the decomposition of O, when the concentration of O, is 5.881×10¯ M? 1/2 Type numbers in the boxes. 10 points hr
Part A Consider the balanced chemical equation. H2O2(aq) + 3I¯ (aq) + 2H+(aq) → I3 (aq) + 2H20(1) Predict the rate of change in the concentration of H2O2 (A[H2O2]/At). In the first 12.0 s of the reaction, the concentration of I drops from 1.000 M to 0.773 M . Express the rate to three significant figures and include the appropriate units. You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. ? A[H2O2]/At = Value Units
What is the order of this reaction with respect to CO ?