Given the following proposed mechanism, predict the rate law for the overall reaction. A_2 + 2B rightarrow 2AB (overall reaction) A) Rate = k[A][B] B) Rate = k[A_2][B] C) Rate = k[A_2][B]^1/2 D) Rate = k[A_2] E) Rate = k[A_2]^1, 2 [B]
At 300 K, the following reaction is found to obey the rate law of Rate = k[NOCl]^2: 2 NOCl(g) 2 NO(g) + Cl2(g) The following reaction mechanism has been proposed for the reaction above: Proposed Mechanism: NOCl(g) ->NO(g) + Cl(g) slow Cl(g) + NOCl(g) -> NOCl(g) fast NOCl2(g) -> NO(g) + Cl2(g) fast 21. The suggested rate law in the mechanism is Rate = k[NOCl]. (T) 22. The reaction mechanism is plausible. (F) 23. NOCl2 is a catalyst in...
For the chemical reaction: A + B 3 C observed to have a rate law of Rate = k [B]2, the following reaction mechanism has been proposed. 2 B D (slow) D + A 3 C + B In your evaluation of the reaction mechanism you would conclude the mechanism is: A) a plausible representation of the reaction B) an implausible representation as the predicted rate law does not match the observed rate law C) an implausible...
The reaction A + 2B → Products was studied and found to have the rate law: Rate = k[A][B]2. By what factor will the rate increase if the concentration of B is tripled while the concentration of A is held constant?
Question 5 and 6 Determine and report the rate law for the reaction of iodide and persul fate ions. Show all calculations and justifications. 2 3.Based on the rate law that you determined above, calculate the values and units of k for: a. the three initial rates experiments in Part A, b. the one initial rates experiment at a different temperature in Part B. 4Use your two experiments done at different temperatures to determine the activation energy Ea and the...
A possible mechanism for the next decomposition reaction is A(g) 2B(g)C (fast equilibrium) 2C +A(g) 2B(g) (slow) What is a rate law that is consistent with this mechanism? Select one: k A B2 k [A]3[B] O a. Rate b. Rate O c. Rate k [A)MB2 O d. Rate k [A3[B2 O f. Rate -k [A/TE] O g. Rate k [A3/[B) h. Rate k [A]3[B]4
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...
Consider the overall reaction and proposed mechanism. What step is rate determining (slow) if the rate law of overall reaction is Rate = k[A][BC] step 1: A + BC --> AB + C step 2: AB + D --> AD + B step 3: B + C --> BC overall reaction: A + D --> AD
4. For the reaction A+B → C+D we find that the rate law is v=k[A]”[B]° Which of the following mechanisms is consistent with the rate law? Explain in detail. a) A+B → C+D b) A+A ~ A2 (fast step) A2 +B → C+D (slow step) c) A+A → A2 (slow step) A2+B → C+D (fast step) d) A+A → A2 (fast equilibrium) A2+B → C+D (slow step)
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....