P.chem A proposed mechanism used to describe the overall chemical reaction A>P is given by A->...
Part A Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast Answer Choices: Rate =...
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]
A chemical reaction, A+B → P, has the following mechanism: 2A< Ki>A, (fast to equilibrium) A+B&K, ™C (fast to equilibrium), A,+C-k>P+ 2A (slow) where Kį and K2 are the equilibrium constants for the first two reactions, respectively. k3 is the rate constant for the third reaction. (a) [5 points] Based on this mechanism, show that the rate of product (P) formation is: d[P] – k[A[B], where k is the rate constant of the overall reaction. Write k in terms of...
Please use the following chemical reaction to explain what is chemical equilibrium, and describe it’s characteristics, in terms of the molar concentrations of the products. [C0450 -(1-ak0,+ acor<o:) Jreactatns products
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....
Molecule A can undergo unimolecular reaction to product P either directly according to mechanism (1) (1) A -> P (k1) or via an intermediate according to mechanism (2): (2) A + M -> A* (k1) A* + M -> A (k2) A* -> P (k3) A. Mechanism 1 If mechanism 1 operates, show that the concentration of [P] vs time is 1st order in [A] B. Mechanism 2 From mechanism (2), derive an expression for the production rate d[P]/dt in...
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...
Name Wkst #16 CHEM& 162 1. Consider the following proposed reaction mechanism. 12 = 21 1 + O₂ → 10₂ + 0 0+ 03 - 202 1 +10, -12 + O2 A. What is the overall reaction? B. What are the intermediates and catalysts? Intermediates: Catalysts: C. If the first step is in equilibrium and the second step is slow. what is the overall rate law? Remember, intermediates cannot appear in the final rate law! Rate = D. On the...
1. The following mechanism has been proposed for the pas-phase reaction of chloroform and chlorine Ch> 20 (fast) CI + CHCI, - HCI +CCI, (slow) Cl + CCI - CCI (fast) a) Identify any intermediate(s): b) Identify any catalyst(s): b) Write the balanced equation for the overall reaction: c) Molecularity of each step: step 1. step 2. step 3 d) rds (circle): 1 2 3 d) What is the observable rate law predicted by this mechanism? e) What is the...
The rate of a chemical reaction can be measured as the rate of appearance of any of the products or as the rate of disappearance of any of the reactants. These relative rates of reaction are related through the stoichiometry of the overall reaction. For example, the rate of the reaction shown below can be determined by measuring the initial rate of disappearance of I, -A[I']/At. CIO3 (aq)91 (aq)+ 6 Ht (aq) 31 3 (aq)CI(aq) 3H20 If the initial rate...