A chemistry graduate student is studying the rate of this reaction:2NH₂ (g) → N₂(g) + 3H₂(g)She fills a reaction vessel with NH, and measures its concentration as the reaction proceeds:time(seconds) [NH]01.00 M0.10 0.699 M0.20 0.489 M0.30 0.342 M0.40 0.239 MUse this data to answer the following questions.Write the rate law for this reaction.Calculate the value of the rate constant k.Round your answer to 2 significant digits. Also besure your answer has the correct unit symbol.rate*-0چار100.0XŚ

Answer: This question is based on trial and error method where we will put the given data in the…

A chemistry graduate student is studying the rate of this reaction: 2NH₂(g) → N₂ (g) + 3H₂(g) She fills a reaction vessel with NH, and measures its concentration as the reaction proceeds: time (seconds) 0 [NH₂] 1.00 M 0.10 0.699 M 0.20 0.489 M 0.40 0.30 0.342 M 0.239 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate k 0 *- 0 7 2 ロ･ロ Xx

A chemistry graduate student is studying the rate of this reaction: 2NH₂(g) → N₂ (g) + 3H₂(g) She fills a reaction vessel with NH, and measures its concentration as the reaction proceeds: time (seconds) 0 [NH₂] 1.00 M 0.10 0.699 M 0.20 0.489 M 0.40 0.30 0.342 M 0.239 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate k 0 *- 0 7 2 ロ･ロ Xx

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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Chemistry 2. The following experimental data are obtained for the decomposition of nitrogen dioxide: 2 NO2(g) → 2 NO(g) + O2(g) ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯ Time, s [NO2], M ln[NO2], [NO2]-1, M-1 ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯ 0 10.0 x 10-3 -4.605 1.00 x 102 60 6.83 x 10-3 -4.986 1.46 x 102 120 5.18 x 10-3 -5.263 1.93 x 102 180 4.18 x 10-3 -5.477 2.39 x 102 240 3.50 x 10-3 -5.655 2.86 x 102 300 3.01 x 10-3 -5.806 3.32 x 102 ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯ Plot a graph of ln[NO2] versus t and 1/[NO2] versus t. Determine the decomposition of NO2 follows a first order or second order rate law with respect to [NO2].
⦁ 2. Explain, in terms of collision theory, why increasing the pressure on the following reaction will probably have very little effect on the reaction rate: 2Al(s)+Fe2O3(s)→2Fe(s)+Al2gO3(s)
O KINETICS AND EQUILIBRIUM Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. N2 H, initial rate of reaction 2.21 M 2.33 M 35.0 M/s 2.21 M 4.98M 160. M/s 7.27 M 2.33 M 379. M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k O k = | Explanation Check O 2021 McGraw-Hill Educ P Type here to search III
For the reaction of : 2 H2O2 (g) → 2 H2O (g) + O2 (g), consider this data table, What is the average rate of reaction between 40 and 50 s for hydrogen peroxide? Time (s) H2O2 (M) 0 1.000 10 0.747 20 0.561 30 0.403 40 0.298 50 0.214 -0.0084 M/s 0.0042 M/s 0.0168 M/s 0.214 M/s 0.0084 M/s
Consider the following reaction mechanism: Step 1: A3(g) → A2(g) + A(g) Step 2: A3(g) + A(g) → 2A2(g) What is the role of A(g) and what is the overall balanced equation? Periodic Table and Datasheet O A(g) is an intermediate; 2A3(g) + A(g) → 3A2(g) + A(g) O A(g) is a catalyst; 2A3(g) + A(g)→ 3A2(g) + A(g) O A(g) is an intermediate; 2A3(g) –→3A2(g) O A(g) is a catalyst; 2A3(g) → 3A2(g)
Given the following balanced equation, determine the rate of reaction with respect to Cl2]. If the rate of Cl2 loss is 4.24 x 10-2 M/s, what is the rate of NO loss? 2NO(g) + Cl2 (g) → 2NOCI(g) O 1.61 × 102 M/s O 8.48 × 10-² M/s O 1.06 × 10-1 M/s O 4.24 x 102 M/s O 2.12 x 10-² M/s
> A Moving to another question will save this response. estion 19 Consider the reaction in aqueous solution: 3r + S20g2- → 13 + 2 SO42- Under a given set of conditions, the concentration of 13 changes from 0,0 M to 7,6 x 10-4 M in 20 seconds. Calculate A[SO2yAt (in mol/L-s) for this time interval. O -6.5 x 10-5 mol/L-s O 5.0 x 10-5 mol/L·s O 1.2 x 10-5 mol/L·s O 7.6 × 10-5 mol/L·s O -5.0 x 105 mol/L-s A Moving to another question will save this response. MacBook Air F6 F5 吕口 F4 F3 F2 F1 #3 24 % 7 6. 4. 2 00
8. Smelling salt decomposes spontaneously at room temperature by the equation below. A student places a 10.00-g sample into a 1-liter sealed rigid vessel. What measurements should the student make to determine the rate of this reaction?(NH4)2CO3(s)→2NH3(g)+H2O(g)+CO2(g) a. change in mass and temperature b. temperature and time c. change in mass and time d. change in pressure and time
The rate of a reaction is how quickly the reaction goes to completion. If two reactions have the same amount of reactant, increasing the rate does not increase the amount of product produced, it simply reduces the time that it takes to make the product. Using the internet , research the four factors below that affect the rate of a chemical reaction. 1. Reactant concentration ( explained with details and add graphs to explain what you wrote for each one of them) 2. pressure ( explained with details and add graphs to explain what you wrote for each one of them) 3. Temperature ( explained with details and add graphs to explain what you wrote for each one of them) 4. Presence of a catalyst. ( explained with details and add graphs to explain what you wrote for each one of them) Your work should be written in complete sentences, and assume your audience is grade 11 chemistry students who do not understand this unit. Make sure all research is put into your own words!
2C1₂0, (g) → 2Cl₂ (g) +50₂ (g) He fills a reaction vessel with C1₂O5 and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 0.20 0.30 [C₁₂05] 0.0500M 0.0322M 0.0207 M 0.0133M 0.40 0.00858M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k [C₁₂0₂] k = 0 x10 □・□ X
A chemistry graduate student is studying the rate of this reaction: She fills a reaction vessel with and measures its concentration as the reaction proceeds: time (seconds) Use this data to answer the following questions. Write the rate law for this reaction. rate Calculate the value of the rate constant . Round your answer to significant digits. Also be sure your answer has the correct unit symbol.
Study the reactions. I. N2 (g) + O2(g) → 2NO(g) II. CO(g) + 02(g) → 2CO2 (g) III. Na(s) + HCI(1) → 2NACI(aq) + H2(g) What factor would only affect the rate of the third reaction? the pressure of the reactants the temperature of the reactants the concentration of the reactants the surface area of the reactants