2) A proposed reaction mechanism for nitric oxide, NO, produced in hydrogen fueled jet engines 1s...
2. Consider the reaction below between nitric oxide and hydrogen gas: 2 NO(g) + 2 H2(g) - N2 + 2 H2009) Upon being studied experimentally, it has been determined that the rate law expression for this reaction is first order in Hz and second order in NO(g). With this information in mind, answer the following: [Tip: You can assume that the steady-state approximation is valid for any intermediate here.) a. As written, is the reaction above a valid mechanism? In...
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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...
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
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
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?
Can you explain with all necessary steps and equations? thank
you
6. The reaction 2 H2 + 2 NO N2 + 2 H20 may proceed by the following mechanism: 2 NO - N202 (k, and k.1) H2 + N202 N2O + H2O (kz) H + N20 - N2 + H2O (ku). Use the steady-state approximation to predict the rate law for the formation of the product N.
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
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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...
20. The reaction of nitric oxide (NO(g)) with a molecular hydrogen (H2(g)) results in the production of molecular nitrogen and water as follows: 2NO(g) + 2H2(g) N20(g)+2H2O(g) According to the following proposed mechanism of this reaction 2NO(g) k-1 (fast equilibrium) N2O2(g) H2(g)+ N2O2(g) N2O(g)+2H20(g) Which of the following is TRUE A) The reaction rate of hydrogen decomposition is consistent with the observed 3rd order. The reaction rate of hydrogen decomposition is consistent with the observed 4th order. B) C) The...
18. The reaction of nitric oxide with hydrogen at 1280°C is: 2 NO (g) + 2 H2 (g) -> N2 (g) + 2 H20 (g) th From the following data determine the rate law and rate constant: Experiment [NO] [H] Initial Rate (M/s) 1 5.0 x 10-3 2.0 x 10-3 1.3 x 10-5 2 10.0 × 10-3 2.0 x 10-3 5.0 x 10-5 10.0 x 10-3 4.0 x 10-3 10.0 x 10-5 3 20 A. Rate = k [NO][H2] B....