4. (22 pts) Consider the following exothermic reaction: H2O2 +2t + 2H' → 12 + 2H20...
8. The rate law for the reaction H2O2 + 2H+212 + 2H2O is rate-k[H202][1]. The following mechanism has been suggested. H2O2+1 - HOI + OH - slow OH + H H20 fast HỘI + H+ + + I2 + H2O fast Identify all intermediates included in this mechanism. A) H and I D) Honly B) H and HOI E) H20 and OH C) HOI and OH 9. Which of the following statements is false? A) A catalyst increases the rate...
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...
For the reaction H2O2 + 2H+ + 2I – ® I2 + 2H2O the following mechanism has been suggested. H2O2 + I – ® HOI + OH – slow OH – + H+ ® H2O fast HOI + H+ + I – ® I2 + H2O fast Identify the rate law for the reaction and explain why
14) You determined the rate law for the reaction of I' with H2O2 in an acidic solution. The rate law was "zero order" with respect to acid ("[H3O+]"). 21+ + H2O2 + 2H+ + 12 + 2 H20 rate = k[I1'[H202] If the conditions are changed to neutral or basic pH, the form of the rate law remains the same but the reaction changes. 2 H2O2 → 2 H2O + O2 rate = k[I+]'[H202] Which statement is TRUE? a) l'...
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 + O2 slow; rate determining step Step 2 NO3 + NO2 --> N2O5 fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. Write the rate law expression for each step of the mechanism including any reversible reactions. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates...
#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2 2Br fast Step 2 Br + H2 H2Br fast Step 3 H2Br + Br 2HBr slow a. What is the overall equation? b. Identify the intermediate(s) if any. c. What is the molecularity and the rate law for each step including any reversible steps? d. What is the predicted rate law expression for this reaction. Be sure to only list reactants from the overall equation and...
Consider the three step reaction mechanism for the atmospheric oxidation in clouds of sulfurous acid to sulfuric acid by hydrogen peroxide H2SO3(9)+ H2O2(9)- H2SO4(9)+ H20(9) Step 1: H2SO3 = HSO3+H* fast Step 2: H202 + H+ = H302 fast Step 3: H302* + HSO3 + H2SO4+H20 slow Which of the following is correct concerning the rate law for the overall reaction? O A. The reaction is first order in each of H2O2 and H2SO3, but of order 0 in H...
The reaction mechanism that has been proposed for the decomposition of H2O2 by iodide ion is: H2O2 + I- → H2O + IO- (slow) H2O2 + IO- → H2O + O2 + I- (fast) Which one of the following statements is true? Select one: a. The reaction is second order with respect to I-. b. I- is an intermediate. c. The reaction is first order with respect to I-. d. IO- is a catalyst. e. The reaction is zero order...
5) rate = K[A][B] Question 11 (1 point) The reaction mechanism proposed for the decomposition of H202 H2O2 + 12 -> H2O + 10-1 (slow) H2O2 + 10-1 --> H2O + O2 + 12 (fast) Which statement is true? 1) The reaction is second order in 1 2) is an intermediate 3) The reaction is first order in and first order in H2O2. 4) 10 1 is a catalyst. 5) The reaction is zero order in ! Question 12110
consider the aqueous reaction of Cl2 + H2S -> S + 2HCL . It may happen by the following mechanism 1: Cl2-> <- 2Cl fast 2: Cl+H2S -> <- HCl + HS fast 3: HS +Cl --> --< HCl + S slow DERIVE a rate law for overall reaction using the given mechanism and rate determining step without using intermediates in the rate law.