![For a certain reaction the rate law is: Rate = k[NO][Cl2]. Which elementary step is the rate limiting step for this reaction?](http://img.homeworklib.com/questions/f52eb090-d736-11ea-b936-ebcb7b2fb289.png?x-oss-process=image/resize,w_560)
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![Rate = KENO] [ch Rate limiting step is rate determined step = slow step. In this reactants are appeared in rate law. Notel NO](http://img.homeworklib.com/questions/f86f3be0-d736-11ea-8a53-11cf2247cf94.png?x-oss-process=image/resize,w_560)
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Can an intermediate appear in the net balanced reaction? Yes, because it is part of the...
Which of the reaction shown is most likely to be an elementary step? CH4 + 202...
Which of the reaction shown is most likely to be an elementary step? CH4 + 202 --> 2H2O + CO2 SO3 + H20 --> H2SO4 Ο Ο Ο Ο N202 + H2 --> N20+H2O C2H4 + H2 --> C2H6
1) 2) 3) A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step...
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A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) N20(g) + H20(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) +H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO2 Ok[NO]2[H212 O k[NO]2[H2] Ok[N20][H2] k[NO]1/2[H2] 2NO(g) +Cl2 (g) → NOCI (8) Experiment concentration of NO (M) 0.09 0.045 0.045 concentration of Cl2(M) Rate (M/s) 0.01 3.40 x 10-4 8.50 x...
2 NO (9) 1. (2 pts) Use the following experimental data to write a Rate Law...
2 NO (9) 1. (2 pts) Use the following experimental data to write a Rate Law for this reaction. Show your work and draw a box around your final answer. + Cl2() + 2 NOCG) [NO] (M) (C12) (M) Initial Rate (Mis) 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 0.50 2. (2 pts) Consider this two-step mechanism for a reaction: Step 1: 2 NO (9) + 2 H2 (9) ** N2 () + H2O2() SLOW Step 2: H2020) +...
Which of the reaction shown is most likely to be an elementary step? CH4 + 202 --> 2H2O + CO2 SO3 + H20 --> H2SO4 Ο Ο Ο Ο N202 + H2 --> N20+H2O C2H4 + H2 --> C2H6
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A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) N20(g) + H20(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) +H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO2 Ok[NO]2[H212 O k[NO]2[H2] Ok[N20][H2] k[NO]1/2[H2] 2NO(g) +Cl2 (g) → NOCI (8) Experiment concentration of NO (M) 0.09 0.045 0.045 concentration of Cl2(M) Rate (M/s) 0.01 3.40 x 10-4 8.50 x...
2 NO (9) 1. (2 pts) Use the following experimental data to write a Rate Law for this reaction. Show your work and draw a box around your final answer. + Cl2() + 2 NOCG) [NO] (M) (C12) (M) Initial Rate (Mis) 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 0.50 2. (2 pts) Consider this two-step mechanism for a reaction: Step 1: 2 NO (9) + 2 H2 (9) ** N2 () + H2O2() SLOW Step 2: H2020) +...
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