8) true. proposed two-step mechanism is shown below. Circle all statements below that are Step 1 (slow): H₂(g) + 2NO(g) N₂O(g) + H₂O(g) Step 2 (fast): N₂O(g) + H₂(g) N₂(g) + H₂O(g) rate, cotla a The overall equation is 2H₂(g) + 2NO(g) b. N₂O(g) is an intermediate. c. N₂(g) is a catalyst. d. Both steps are bimolecular. e. The rate law for step 1 is rate = k[H₂][NO] f. The rate law for the overall reaction is rate = k[H₂][NO]² => N₂(g) + 2H₂O(g). 1 [H₂] [A10] ² → W[0₂0] [H 7) from 2.50 s¹ at a temperature of 22.0°C to 12.5 s¹ at a temperature of 35.0°C. Calculate the activation energy, in kJ/mol, for a given reaction if the rate constant increases

8) true. proposed two-step mechanism is shown below. Circle all statements below that are Step 1 (slow): H₂(g) + 2NO(g) N₂O(g) + H₂O(g) Step 2 (fast): N₂O(g) + H₂(g) N₂(g) + H₂O(g) rate, cotla a The overall equation is 2H₂(g) + 2NO(g) b. N₂O(g) is an intermediate. c. N₂(g) is a catalyst. d. Both steps are bimolecular. e. The rate law for step 1 is rate = k[H₂][NO] f. The rate law for the overall reaction is rate = k[H₂][NO]² => N₂(g) + 2H₂O(g). 1 [H₂] [A10] ² → W[0₂0] [H 7) from 2.50 s¹ at a temperature of 22.0°C to 12.5 s¹ at a temperature of 35.0°C. Calculate the activation energy, in kJ/mol, for a given reaction if the rate constant increases

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.92QE

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