Clearly the third step is the slowest step and thus it is the rate determining step . The rate law expression has been solved in the given figure above..
8. Find the rate law of the reaction: keff 3HNO2 H2O + 2NO + H+ +...
- For the reaction 2NO + O2 + 2NO the following reaction mechanism have been suggested; steps: NO + NON2O2 Fast step 2: N2O2 + O2 k2 2NO Slow and the apparent rate law was found to be R = kerr [NO] What would be the estimated effective activation energy, El. value, if the activation energies for forward and backward reactions in step 1 are 82 kJ mol" and 205 kJ moll, respectively, and the activation energy of step 2...
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...
please help:) thank you 58 The rate for the following to be 0.22M NO2 I min. w rate at 320K? ollowing reaction at book was found 102 1 min. what would be the approximate N204 Lg) - ZNO2Lg) the following rate St. A reaction occurs in three steps with constants: KI=0. 3M K2=0.05M, Step 1 (a) which step is the slow step? AK D 3M B K2=00SM ( +3=4.5MD Ck3=4.50 Step 2 Step 3 (b) which step has the lowest...
Select all that apply. The rate law for the reaction 2NO(g) + Cl2(g) → 2NOCI(g) is given by R-k[NO][C121 If the following is the mechanism for the reaction, NO(g) + Cl2(g) → NOC12(g) NOCI,(g) + NO(g) → 2NOCI(g) which of the following statements accurately describes this reaction? Check all that apply. 2nd order reaction The first step is the slow step. Doubling [NO] would quadruple the rate. Cutting (Cl) in half would decrease the rate by a factor of two....
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...
Reaction Mechanism Review CHM 1120 NO + H₂ + N + NON +H2O + N2O step 1 NO+Hp --> N + H2O (slow) step 2 N+NO --> NO ZNO + H2H₂O + N2O bimolecular Unimolecular Rate = K[NO] + [tz step 1 NO-NO-> NO: +sowotworola + H 2 + 8 + 16 - JÓz + x + 46 +H2O + N20 step 2. step 3 NO2 + H2 --> NO + H2O N+NO -> NO ZNO +H2 H2O + N20...
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
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
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
For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: O3(g)+2NO2(g)→N2O5(g)+O2(g) Step 1: O3(g)+NO2(g)→NO3(g)+O2(g) slow Step 2: NO3(g)+NO2(g)→N2O5(g) fast View Available Hint(s) For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: Step 1: slow Step 2: fast A.] Rate=k[O3][NO2]2 B.] Rate=k[O3][NO2] C.] Rate=k[NO3][NO2] D.] Rate=k[O3][NO2]2[N2O5][O2]