Given this data in a study on how the rate of areaction was affected by the concentration of thereactants (Show work on separate page for the restof the exam and submit in assignments)run [A][B][C] rate, M/hr10.2000.1000.6005.020.2000.4000.40080.030.6000.1000.20015.040.2000.1000.2005.050.2000.2000.40020.0a) Give the rate law.b) Give the rate constant.

Answered: Image /qna-images/answer/bc842388-292f-4831-ae8e-0415d2e2f010.jpg

Answered: Given this data in a study on how the…

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

(a) A study was made of the effect of hydroxide ion, OH–, concentration on the rate for the following reaction: I–(aq) + OCl–(aq) ----------------> IO–(aq) + Cl–(aq) Experimental data: [I] [OCl–] [OH–] Rate M/sec 0.0013 0.012 0.1 9.4 x 10-3 0.0026 0.012 0.1 18.7 x 10-3 0.0013 0.006 0.1 4.7 x 10-3 0.0013 0.018 0.1 14.0 x 10-3 0.0013 0.012 0.05 18.7 x 10-3 0.0013 0.012 0.2 4.7 x 10-3 0.0013 0.018 0.2 7.0 x 10-3 Determine the rate law and the value of the rate constant, k.
0.003 0.00243 0.002 M 0.001 5 10 15 20 25 30 seconds created Is C,H,OH being created or destroyed by the chemical destroyed reaction? neither created nor destroyed If C,H,OH is being created or destroyed, what is the rate at which it is being created or destroyed 13 seconds after the reaction starts? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. If C,H,OH is being created or destroyed, what is the average rate at which it is being created or destroyed during the first 13 seconds of the reaction? O O
1) 2 H,Oz (aq) → 2 H2O (l) + Oz (g) Time (s) 0 10 20 30 40 50 60 70 80 [H₂O₂] (M) 1.00 0.75 0.55 0.40 0.30 0.22 0.18 0.12 0.10 Use the experimental data for the above reaction to answer. a) What is the average rate of disappearance of H₂O₂ between 30 and 40 seconds? b) What is the average rate of reaction between 50 and 70 seconds? c) What is the average rate of formation of O₂ between 40 and 60 seconds?
Consider the following reaction and information: A + 2B → 3C rate = k{B} Time (min.) B (M) A (M)0 0.72 0.5030 0.25 0.2660 0.087 0.18 What is the concentration of B after 27 minutes?
The following images depict the evolution of the chemical reaction A → B over time: B Part A A- t=0 s Compare the reaction A → B to the reaction Y→ Z. Which reaction has the faster rate? Y→Z t = 20 s t=0 s t = 20 s t = 40 s t = 40 s t = 60 s t = 60 s A B Y Z ●
Question 2 options: The balanced equation for a given reaction is X + Y → P. The following data regarding initial reaction rates were collected in the lab. Fill in the blanks regarding this reaction by typing the correct number without units. Trial [X] (M) [Y] (M) Rate (M/s) 1 0.020 0.060 3.40 x 10–3 2 0.020 0.120 2.72 x 10–2 3 0.080 0.060 1.36 x 10–2 What is the order with respect to X? What is the order with respect to Y? What is the overall order of the reaction? What is the rate constant, k, written to 3 significant figures?
How did the rate change when the reaction was performed at a higher temperature? why? expalin at the molecular practice level.
A Stay goggles while performing the experiment. Part A In this task, you'll observe a chemical reaction between baking soda and vinegar. How do you think the temperature of the reactants and the rate of reaction are related? Write a hypothesis to predict the relationship between the two parameters. B IU x X, Font Sizes A - Characters used: 0/ 15000 Part B
4. The following data were obtained for the follwing chemical reaction: 2A + 3B ---> 2C + D Initial [A] Initial [B] Initial Rate of Formation Trial # (mmol/L) (mmol/L) of D (mmol/L*s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (b) Find the rate constant, k, with units.
1. In the Rates of Chemical Reactions lab you measured the experimental rate of the following reaction: S208 +212 +2 SO4² Given a graph of moles S₂Og 2 consumed versus time (s) with a best fit linear line and a total volume of 325 mL for the reaction, explain how would you determine the rate of reaction? 2. The initial rates listed in the following table were determined for the reaction: H2PO3 (aq) + OH (aq) →HPO3²¯ (aq) + H2O (1) Trial Initial [H₂PO3¯], (M) Initial [OH], (M) Initial Rate of Consumption (M/s) 1 0.025 0.030 0.432 2 0.100 0.030 1.728 3 0.100 0.015 0.864 a) What is the rate law? b) What is the value of the rate constant, k? c) What is the initial rate when the initial concentrations of both reactants are 0.12 M? 3. The following experimental data was obtained for the bromination of acetone at 30°C. 21 +2 H+H2O2 → I2 + 2 H₂O Trial Initial [I] (M) Initial [H+] Initial [H2O2] (M) Rate (M/sec) (M) 1 0.001 0.005 0.001 2.0 x 104 2 0.002 0.005 0.001 4.0 x 10+ 3 0.006 0.002 0.001…
Last part of this question... An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 → 2NH3. Starting with a closed reactor containing 1.25 mol/L of N2 and 0.35 mol/L of H2, she finds that the H2 concentration has fallen to 0.12 mol/L after 40. seconds. What is the average rate of reaction of H2 over this time? (Enter in mol/liter/sec). 0.0058 You are correct.Your receipt no. is 155-176 Previous Tries What is the average rate of NH3 production for this example? (Enter in mol/liter/sec). 0.0038 You are correct.Your receipt no. is 155-8777 Previous Tries Estimate the N2 concentration after 40 seconds? (Enter in mol/liter).
Please answer this question

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS