Given the following proposed mechanism:
A3 ⇌ A2 + A K1, fast step
A + A3 → 2A2 k2, slow step
The rate rate law is Question 5 options:
a.)second order in A3 and first order in A2
b.)second order in A3 and zero order in A2
c.)first order in A3 and zero order in A2
d.)inverse order, i.e., -1, in A3 and second order in A2
e.)second order in A3 and inverse order, i.e., -1, in A2
f.)zero order in A3 and second order in A2
g.)first order in A3 and first order in A2
Given the following proposed mechanism: A3 ⇌ A2 + A K1, fast step A + A3...
The rate law for the mechanism below is A2(g) ⇌ 2A(g) K1, fast A(g) + B(g) ⇌ AB(g) K2, fast AB(g) + A(g) → A2B(g) k3, slow Options: rate = K2k3[A]2[B] rate = K1K2k3 [A2][B] rate = K10.5k3 [A2]0.5[AB] rate = k3[A][AB] rate = K10.5K2k3 [A2]0.5[A] [B]
For the following two-step mechanism: Step 1: NO (g) + NO (g) --K1--> N2O2 (g) (fast, equilibrium) <------- Step 2: N2O2 (g) + Br2 (g) ------> 2 NOBr (g) (slow) (a) Write the equation for the overall reaction. (b) Write the raw law for the overall reaction.
For a reaction that proceeds by the following two-step mechanism A2 ⇄ 2A (fast) A + B → C (slow) Which of the following statements is/are correct? 1) The reaction is first order in the concentration of A2. 2) B is a reaction intermediate. 3) The rate-determining step is bimolecular. 4) The units of the specific rate constant are mol1/2L-1/2s-1
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....
The following mechanism has been proposed for the gas-phase reaction of H2 with ICl: H2(g)+ICl(g)→HI(g)+HCl(g)HI(g)+ICl(g)→I2(g)+HCl(g) c) Write rate laws for each elementary reaction in the mechanism?Use a for [H2], b for [ICl] and k1 for the rate constant. d) Use c for [HI], d for [ICl] and k2 for the rate constant? e) If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction? Use a...
Predict the overall reaction from the following two-step mechanism: 2 A→A 2(fast) A2+B→A2B(slow) Express your answer as a chemical equation. Predict the rate law from the following two-step mechanism: 2A⇌ A2 (fast) A2+B→A2B (slow)
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...
Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1 Step 2: NO(g) + ) --> NO2 (g) rate = k2 suppose that k1<<k2, That is the first step is much slower than the second. Write the balanced chem equation for the overall chemical rxn Write the experimentally observable rate law for the overall reaction. (no reaction concentrations) rate=k() Express the rate constant k for the overall reaction in terms of k1, k2 and (if necessary) the rate constant...
4. Below is a proposed mechanism for a reaction: Step 1. Step 2. C+E-F Step 3. F G A B C+D Fast equilibrium Slow Fast A. (2 points) What is the overall stoichiometry for this reaction? B. (2 points) Which step is the rate determining step? C. (6 points) If this mechanism is correct, what should the rate equation for this reaction be? (Make sure you include the fast equilibrium)
Question 5 (1 point) Saved The rate law for the mechanism below is A260) = 2A K1, fast Bu + 2A - A2B K2, fast A2B + Bus -- 2AB k3, slow Orate = K10.5 K2k3 [A2]0.5[B]2 rate = K1 K2k3 [A2][B]2 rate = k3|A2B][B] rate - Kyk3[A]”[B]2 rate - Kyk31A)?(B)