A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) →...
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
1) 2) 3) 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...
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 experimental rate law for the reaction 2H2(g) + 2 NO(g) → N2(g) +2 H2O(g) is d[N2) = kods[Hz][NO] Below is a proposed mechanism: H2(g) + NO(g) + NO(g) = N2O(g) + H2O(g) H2(g) + N2O(g) = N2(g) + H2O(g) ki k2 (a) Under what conditions does this mechanism give the observed rate law? Express kobs in terms of the rate constants for the individual steps of the mechanism. A second proposed mechanism is: NO(g) + NO(g) = N2O2(g) N2O2(g)...
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...
The rate law for the reaction 2H2(g) + 2NO(g) ----> N2(g) + 2H2O(g) is rate=k[H2][NO]2. What is the rate constant at 800 degrees C when [NO] = 0.050 M and [H2] = 0.010 M and the rate of the reaction is 1.5 M/s
For the reaction, 2NO(g)+2H2(g)→N2(g)+2H2O(g), what direction will the reaction proceed if [NO]=7.9x10-3M, [H2]=0.25 M, [N2]=0.15 M, & [H2O]=0.13 M. (K=650) forward reverse the reaction has stopped the reaction is at equilibrium
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...
2) A proposed reaction mechanism for nitric oxide, NO, produced in hydrogen fueled jet engines 1s 2 NO(g) N202(g) N202(g) + H2(g) H20(g) +N20(g) N20(g) +H2(g) N2(g) + H20(g) fast slow fast a) Write a balanced equation for the overall chemical reaction (1/2 mark) b) Determine the theoretical rate law. (1 mark) c) Using the blank reaction progress diagram below sketch the energy profile of this exothermic reaction mechanism, labeling the positions of NO. H2,N 02, N2O, H2O, N2. (3...