A proposed mechanism for a reaction is: C₂H₂Br C₂H₂+ + Br C₂H₂+ + H₂O C₂H₂OH₂+ C₂H₂OH₂+ + H₂O a) What is the overall chemical equation for the reaction mechanism? b) What is (are) the intermediate(s)? c) If a catalyst was added to this reaction mechanism, which step should it target for maximum impact? EXPLAIN. - (slow) (fast) C₂H₂OH + H₂O+ (fast)

A proposed mechanism for a reaction is: C₂H₂Br C₂H₂+ + Br C₂H₂+ + H₂O C₂H₂OH₂+ C₂H₂OH₂+ + H₂O a) What is the overall chemical equation for the reaction mechanism? b) What is (are) the intermediate(s)? c) If a catalyst was added to this reaction mechanism, which step should it target for maximum impact? EXPLAIN. - (slow) (fast) C₂H₂OH + H₂O+ (fast)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Ch. 14, 54. A reaction indicated by the chemical equation below was monitored as a function of time: AB → A+B A plot of 1/[AB] versus time yields a straight line with a slope of 0.055 M-¹ s-¹. a) Determine the rate constant for this reaction (assume the temperature does not change). b) Write the rate law equation for the reaction. c) What is the half-life of the reaction if the initial concentration of AB is 0.550 M? d) If the initial concentration of AB is 0.250 M, what are the molar concentrations of A and B after 75 s?
Question 4 Calculate the frequency factor (A). Studies have shown that the reaction occurs via the following mechanism. ki Cl2O4 k-1 Step 1: 2 Cl02 (fast equilibrium) k2 Step 2: C2O4 + OH- → ClO;¯+HCIO2 (slow) k3 Step 3: HCIO2 + OH → ClO2¯+H2O (fast) Question 5: Identify the intermediate/s and the rate-determining step. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 → ClO3¯+HC1O2 Step 2: C204 + OH- (slow) k3 Step 3: HC1O2 + OH- ClO2- + H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 Step 2: C204 + OH- → ClO3¯+ HCIO2 (slow) k3 Step 3: HCIO2 + OH- → ClO2-+ H2O (fast) Question 7 Draw the transition state for Step 3. Identify the bond/s forming/breaking.
for the following mechanism proposed wfor the decomposition of hydrogen peroxide using potassium bromide (see image) which of the following reactuin intermediates
For the following chemical Konction there are possible Reaction mechanisms as Shown STEP I Step 2 NET 2 co + Cl₂ → 2 Coll STEP 1 Step 2 REACTION MECHANISM I со - CO + Cl₂ ⇒ Coll + el C(Slow) (Fast) со coel اح tee Three MECHANISM I Cl₂ → 2 l (Slow) llz 2 ll + 10 + 2 coll (Fast)
1) The reaction order with regards to nitrogen monoxide gas is : The reaction order with regards to hydrogen gas is : 2) The student performs Trial 4 with the same initial concentrations as Trial 1 but a higher temperature. The initial rate of Trial 4 should be : a) equal to b) higher than c) lower than Trial 1. The student forms performs Trial 5 with initial concentrations of both reactants of 0.20M. The initial rate of Trial 5 should be a) equal to b) higher than c) lower than Trial 1
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Mechanism Suppose a reaction occurs with the following mechanism. All are elementary steps. Step 1: 0₂(9) 20(g) fast K₂ Step 2: O(g) + N₂(g) Step 3: O(g) + N(g) گی 3 NO(g) + N(g) slow very fast K3, NO(g) $ 4 % 5 6 What is the rate law for the rate-determining step? Rate =k,[0₂]² Rate = kr[O]² Rate-k,[O][N] Rate = kf[0₂]/k,[0]² Rate = k₂[O][N₂] Rate = K[0₂] & 7 What is the rate law for the forward reaction in step 1? Rate = kr[O]² Rate = kr[0₂] Rate =k+[0₂1² Rate = kr[0₂1² Rate = kf[0]² Rate =k+[0₂] What is the overall rate law for this reaction? Rate = k[N₂][0₂][N][0] MacBook Pro 8 ( 9 ☆ 88