![5) rate = K[A][B] Question 11 (1 point) The reaction mechanism proposed for the decomposition of H202 H2O2 + 12 -> H2O + 10-1](http://img.homeworklib.com/questions/05324d30-e017-11eb-a0a9-6d594e977d3d.png?x-oss-process=image/resize,w_560)
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5) rate = K[A][B] Question 11 (1 point) The reaction mechanism proposed for the decomposition of...
The reaction mechanism that has been proposed for the decomposition of H2O2 by iodide ion is:...
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...
The following mechanism, proposed for the decomposition of hydrogen peroxide is composed of 2 elementary steps:...
The following mechanism, proposed for the decomposition of hydrogen peroxide is composed of 2 elementary steps: H2O2(aq) + I'(aq) > H2O(l) + 10 (aq) 10 (aq) + H2O2(aq) -> H2O(l) + O2(g) + I'(aq) The rate law predicted by the mechanism is slow fast a) rate = k [H2O2) b) rate =k [H202][I] c) rate =k [H2O2][10] d) rate = k [H202) [1]
The decomposition of hydrogen peroxide (H2O2(aq)) is proposed to follow a reaction mechanism of Step 1:...
The decomposition of hydrogen peroxide (H2O2(aq)) is proposed to follow a reaction mechanism of Step 1: H2O2(aq) + Br(aq)-H2O(l) + BrO (aq) Step 2: Bro (aq) + H2O2(aq),H2O(l) + O2(g) + Br(aq) What is the catalyst, and what is the effect of having a catalyst present? Periodic Table and Datasheet Br is the catalyst, and the reaction follows a faster pathway with Br than without BrO is the catalyst, and the reaction follows a faster pathway with Bro-than without Bro...
6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction...
6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: O:(g) + O(g) →202(g): rate = k[O][NOJ Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: H2O2(aq) + I'(aq) → H2O(l) + Of(aq) ---...-slow H2O2(aq) + Or(aq) → H2O(0) + O2(g) + I'(aq) -----fast What...
QUESTION 21 A proposed mechanism for the decomposition of ozone in the atmosphere is: Step 1:...
QUESTION 21 A proposed mechanism for the decomposition of ozone in the atmosphere is: Step 1: 03(g) + hv → O(g) + O2(g) Step 2: O(g) + O3(g) → 202(0) Does this reaction mechanism have an intermediate and/or catalyst? Only a catalyst Only an intermediate An intermediate and a catalyst More information is needed O Neither an intermediate nor a catalyst
13.108. 13.109. 13.102. A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary...
13.108. 13.109. 13.102. A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps: H2O2(g) + 2 OH(g) H2O2(g) + OH(g) → H2O(g) + HO2(g) HO2(g) + OH(g) → H2O(g) + O2(g) පිපිළි 13.110. If the rate law for the reaction is first order in H2O2, which step in the mechanism is the rate-determining step?
14) You determined the rate law for the reaction of I' with H2O2 in an acidic...
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'...
i. For the reaction: 2H202→ 2H2O+O2 a proposed mechanism is: H2O2 + H3O2+ → H2O +...
i. For the reaction: 2H202→ 2H2O+O2 a proposed mechanism is: H2O2 + H3O2+ → H2O + H30+ +02 (a) The intermediate in the proposed mechanism is The catalyst is (b) Apply the steady state approximation to this mechanism to deduce the rate law in terms of d[O2]/dt. (15 pts)
QUESTION 10 A proposed mechanism for the decomposition of ozone in the atmosphere is: Step 1:...
QUESTION 10 A proposed mechanism for the decomposition of ozone in the atmosphere is: Step 1: 03(g) + hvO(g) + O2(g) (fast) Step 2: O(g) + O2(g) +202() (slow) What is the molecularity of the rate-determining step? unimolecular bimolecular zeromolecular More information is needed. termolecular QUESTION 11 At a certain temperature the equilibrium equals 0.11 for the reaction: 2 ICI(g) =12(g) + Cl2(g). What is the equilibrium concentration of Cl2 if 2.78 mol of 12 and 2.78 mol of Cl2...
1. The mechanism for hydrogen peroxide decomposition is thought to occur in two step: step 1:...
1. The mechanism for hydrogen peroxide decomposition is thought to occur in two step: step 1: H2O2+ I ------> IO + H2O step 2: IO + H2O2 --------> I + H2O + O2 a. describe each step in the mechanism as unimolecular ,bimolecular or termolecular ? b. which species in the mechanism acts as an intermediate.? c. which species in the mechanism acts as catalyst.? d. what is the net reaction?
The following mechanism, proposed for the decomposition of hydrogen peroxide is composed of 2 elementary steps: H2O2(aq) + I'(aq) > H2O(l) + 10 (aq) 10 (aq) + H2O2(aq) -> H2O(l) + O2(g) + I'(aq) The rate law predicted by the mechanism is slow fast a) rate = k [H2O2) b) rate =k [H202][I] c) rate =k [H2O2][10] d) rate = k [H202) [1]
The decomposition of hydrogen peroxide (H2O2(aq)) is proposed to follow a reaction mechanism of Step 1: H2O2(aq) + Br(aq)-H2O(l) + BrO (aq) Step 2: Bro (aq) + H2O2(aq),H2O(l) + O2(g) + Br(aq) What is the catalyst, and what is the effect of having a catalyst present? Periodic Table and Datasheet Br is the catalyst, and the reaction follows a faster pathway with Br than without BrO is the catalyst, and the reaction follows a faster pathway with Bro-than without Bro...
6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: O:(g) + O(g) →202(g): rate = k[O][NOJ Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: H2O2(aq) + I'(aq) → H2O(l) + Of(aq) ---...-slow H2O2(aq) + Or(aq) → H2O(0) + O2(g) + I'(aq) -----fast What...
QUESTION 21 A proposed mechanism for the decomposition of ozone in the atmosphere is: Step 1: 03(g) + hv → O(g) + O2(g) Step 2: O(g) + O3(g) → 202(0) Does this reaction mechanism have an intermediate and/or catalyst? Only a catalyst Only an intermediate An intermediate and a catalyst More information is needed O Neither an intermediate nor a catalyst
13.108. 13.109. 13.102. A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps: H2O2(g) + 2 OH(g) H2O2(g) + OH(g) → H2O(g) + HO2(g) HO2(g) + OH(g) → H2O(g) + O2(g) පිපිළි 13.110. If the rate law for the reaction is first order in H2O2, which step in the mechanism is the rate-determining step?
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'...
i. For the reaction: 2H202→ 2H2O+O2 a proposed mechanism is: H2O2 + H3O2+ → H2O + H30+ +02 (a) The intermediate in the proposed mechanism is The catalyst is (b) Apply the steady state approximation to this mechanism to deduce the rate law in terms of d[O2]/dt. (15 pts)
QUESTION 10 A proposed mechanism for the decomposition of ozone in the atmosphere is: Step 1: 03(g) + hvO(g) + O2(g) (fast) Step 2: O(g) + O2(g) +202() (slow) What is the molecularity of the rate-determining step? unimolecular bimolecular zeromolecular More information is needed. termolecular QUESTION 11 At a certain temperature the equilibrium equals 0.11 for the reaction: 2 ICI(g) =12(g) + Cl2(g). What is the equilibrium concentration of Cl2 if 2.78 mol of 12 and 2.78 mol of Cl2...
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