**Question 12**Using the data in the following table, calculate the average rate of the reaction:\[ 2NO_2(g) \rightarrow 2NO(g) + O_2(g) \]| Time (s) | [NO₂] ||----------|----------------|| 0 | 0.125 M || 520 | 0.098 M |Options:- (a) \(1.9 \times 10^{-4} \, \text{M/s}\)- (b) \(2.6 \times 10^{-5} \, \text{M/s}\)- (c) \(5.2 \times 10^{-5} \, \text{M/s}\)- (d) \(2.4 \times 10^{-4} \, \text{M/s}\)---**Question 13**The following graphs can be used for the questions that follow: [Graph not provided in image]

12. Given that : We have to calculate the average rate of the reaction : 2NO2(g) → 2NO(g) +…

Answered: QUESTION 12 Using the data in the…

Chemistry

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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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The following data was collected for the reaction 3 H2 + N2 2 NH3. Time (s) [H2] (M) 1.00 10 0.75 Based on these data, what is the average rate of the reaction in the time period from 0 s to 10 s? O 0.0125 M/s 0.025 M/s O -0.025 M/s 0.050 M/s 0.00833 M/s 0.075 M/s
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QUESTION 30 In the reaction 2 H₂O2(aq) → 2 H₂O() + O2(g), the initial concentration of H₂O2 is 0.600M and, 28.4 seconds later, the concentration of H₂O2 is 0.330 M. What is the average rate of reaction over this time interval? O a. 0.0116 M/s O b.-0.00475 M/s OC. 0.00475 M/s O d.-0.0095329 M/s O e. 0.0095903 M/s
2
QUESTION 2 The following mechanism has been proposed for the gas-phase exothermic reaction of chloroform (CHCl3) and chlorine: Step 1: Step 2: Step 3: Q 2(a) Cl₂2Cl Cl + CHCl3 → HCl+ CCl3 Cl + CCl3 → CCl4 i. What is the overall reaction? (fast) (slow) (fast) ii. What are the intermediates in the mechanism? iii. What is the molecularity of the elementary reactions? iv. Write down the rate law for each elementary reaction. v. What is the rate-determining step? Q 2(b) Using the rate-determining step and pre-equilibria determine the rate law predicted by this mechanism. Q2(c) Roughly sketch and label a reaction profile graph (potential energy vs reaction coordinate) for this reaction. ii. Include in the graph: reactants, products, intermediary/intermediaries, activation energy for each elementary step. iii. Compare the activation energy for all the elementary step, indicating which one is the highest.
QUESTION 13 Given the reaction 2N 20 5(g) → 4NO 2(g) + O 2(g), the rate of reaction based on N 20 5(g) is correctly written as ate ate = - 2 %3D ate = rate = - AN205] Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Air
Question 9 Which of the following statements is false? The average rate of a reaction decreases during a reaction. It is not possible to determine the rate of a reaction from its balanced equation. The rate of zero order reactions is not dependent on concentration. The half-life of a first order reaction is dependent on the initial concentration of reactant. None of the statements are false.
HI dissociates to form I2 and H2: 2 HI(g) → H2(g) + I2{g) If the concentration of HI changes at a rate of -0.45 M/s, what is the rate o appearance of l2(g)? 0.45 M/s O 0.13 M/s O 0.23 M/s O 1.00 M/s O 0.90 M/s

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QUESTION 12 Using the data in the following table, calculate the average rate of the reaction 2NO 2(g) 2NO(g) + O 2(g). Time(s) [NO2] 0. 0.125 520 0.098 1.9 x 10-4 M/s 2.6 x 10-5 M/s 5.2 x 10-5 M/s 2.4 x 10-4 M/s