The formation of hydrazine N2H4(g) follows the proposed mechanism:
Step I) N2 + H2 → N2H2
Step II) H2 + N2H2 → N2H4
If the second step is the slow step, write the rate law for the overall reaction. Show your work.
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The formation of hydrazine N2H4(g) follows the proposed mechanism: Step I) N2 + H2 → N2H2...
The following mechanism has been proposed for the formation of hydrazine in the overall reaction, ?2 (?) + ?2 (?) → ?2?4 (?): ???? 1: ?2 + ?2 → ?2?2 ???? 2: ?2 + ?2?2 → ?2?4 The rate law for the overall reaction is ???? = ?? [?2 ][?2]2. Which step is the slow step? Show your work.
QUESTION 19 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) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO]1/2[H2] k[NO]2[H2] k[NO] [H2)2 k[N20][H2] k[NO]2
QUESTION 9 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) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? k[N2O][H2] k[NO]2[H2] k[NO]2[H2]2 k[NO]1/2[H2] k[NO]2
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) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? O k[no]/2[Hz] O k[N20][H2] O k[NO]2 O k[NO]2[Hz] O k[NO]2[H212
1. A proposed mechanism for a reaction is: 1221 (rapid equilibrium) I + H2 = H2 (rapid equilibrium) H21 + 1 = 2 HI (slow) a. Write the overall balanced equation for this reaction. (4 pts.) b. Indicate which step is the rate determining step. (1 pt.) c. Based on the mechanism proposed, write the rate law for the overall reaction. (2 pts.) d. Using ki, ki, ka, etc., write the value for the overall rate constant k. (2 pts.)...
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
Please answer each part with work shown. Thank you. 6. The following three mechanisms have been proposed for a particular reaction. Mechanism II Mechanism III Mechanisml H2 +NO-H2O+N (slow) N +NON2+0 (fast) O+H2-> H2O (fast) 2 NO-N202 (fast equilibrium) H2-N202-H20+ N3O (slow) H2+N20-H2O+N2 (fast) H2 + 2 NO- H2O+N2O (slow) N20+ H2N2+ H2O (fast) a) What is the overall reaction that each proposed mechanism supports? b) Calculate the ΔΗ'm for the overall reaction. c) For each mechanism, draw an energy...
14. The reaction 2 H2(g) + 2 NO(g) ® N2(g) + 2 H2O(g) is proposed to have the alternate mechanism: 2 NO(g) ® N2O2(g) FAST N2O2(g) + H2(g) ® N2O(g) + H2O(g) SLOW N2O(g) + H2(g) ® N2(g) + H2O(g) FAST If the rate law is found to be Rate = k[H2][NO]2, could this support the proposed mechanism? Does the rate law indicate that the reaction is termolecular?
The following mechanism has been proposed for the gas-phase reaction of H2 with ICl: H2(g)+ICl(g)→HI(g)+HCl(g)HI(g)+ICl(g)→I2(g)+HCl(g) c) Write rate laws for each elementary reaction in the mechanism?Use a for [H2], b for [ICl] and k1 for the rate constant. d) Use c for [HI], d for [ICl] and k2 for the rate constant? e) If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction? Use a...
What is the equation for the formation reaction for gaseous hydrazine, N2H4, at 25°C and 1 atm pressure? O 2N2H4(9) — 2NH3(g) + H2(g) O 2NH3(9) + H2(g) – N Ha(g) O N2(g) + 2H2010) – N2H4 (9) * 0219) O N2(g) +2H2(0) – N2Halg) O 2N02/9+ 6H219) -- NąHal9) 4H2010)