![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)](http://img.homeworklib.com/questions/8002f880-c6c2-11ea-8058-659c95878d31.png?x-oss-process=image/resize,w_560)
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i. For the reaction: 2H202→ 2H2O+O2 a proposed mechanism is: H2O2 + H3O2+ → H2O +...
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 reaction 2 H202 + 2H2O + O2 has the following mechanism: H2021H2010 H2O2 +10 H2O...
The reaction 2 H202 + 2H2O + O2 has the following mechanism: H2021H2010 H2O2 +10 H2O + O2 + 1" Are there any catalyst? If so, what are they? Are there any intermediates? If so, what are they? Equilibrium Basics (14 Points) The reaction: Hi(9) 1(9) = 2HI(9) has Kp = 459 at 763 K. A particular equilibrium mixture at 763K contains gaseous Hl at a partial pressure of 4.00 atm and hydrogen gas at a partial pressure of 0.229...
4. Now consider the catalase catalyzed decomposition of hydrogen peroxide to water. The much needed catalyst....
4. Now consider the catalase catalyzed decomposition of hydrogen peroxide to water. The much needed catalyst. 2H202 + catalase → 2H2O + O2 + catalase a. [3] Assume the following mechanism: H2O2 + catalase = {H202-catalase} HIS 54 Inhibitor ASN 127 H2O2 + {H202-catalase} → catalase + 2H20 + O2 Oxygen When the pre-equilibrium approximation is used, the rate-law is: 41 dt Kegk2[H202]?[E]. The steady-state approximation gives a more general rate law. Derive the rate law using the SS approximation....
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 + 0 + M 0+03 2 02 Apply the steady-state approximation to the concentration of atomic oxygen, and derive t...
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 + 0 + M 0+03 2 02 Apply the steady-state approximation to the concentration of atomic oxygen, and derive the rate law for the decomposition of ozone (M stands for a molecule that can exchange kinetic energy with particles undergoing the chemical reaction.)
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 +...
For the reaction H2O2 + 2H+ + 2I – ® I2 + 2H2O the following mechanism...
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
H2O2 + 3 I- + 2 H+ → I3- + 2 H2O Step 1. H2O2 +...
H2O2 + 3 I- + 2 H+ → I3- + 2 H2O Step 1. H2O2 + H+ → H3O2+ Step 2. H3O2+ + I- → H2O + HOI Step 3. HOI + I- → OH- + I2 Step 4. OH- + H+ → H2O Step 5. I2 + I- → I3- How many of the following statements are correct based on the information given? 1. I3- is a product of this reaction 2. I2 is a reactant in this reaction...
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...
Question 8 Step 1: H,02 + I +10- +H,0 Step 2: H,02 + 10 + H2O...
Question 8 Step 1: H,02 + I +10- +H,0 Step 2: H,02 + 10 + H2O + O2 +I" The mechanism for a chemical reaction is shown above. Which of the following statements about the overall reaction and rate laws of the elementary reactions is correct? The chemical equation for the overall reaction is 2 H202 + I and the rate law for elementary step 2 is rate = k[H,02][10 + 2 H2O + O2 +I , ]. + H2O...
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'...
5) rate = K[A][B] Question 11 (1 point) The reaction mechanism proposed for the decomposition of...
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
The reaction 2 H202 + 2H2O + O2 has the following mechanism: H2021H2010 H2O2 +10 H2O + O2 + 1" Are there any catalyst? If so, what are they? Are there any intermediates? If so, what are they? Equilibrium Basics (14 Points) The reaction: Hi(9) 1(9) = 2HI(9) has Kp = 459 at 763 K. A particular equilibrium mixture at 763K contains gaseous Hl at a partial pressure of 4.00 atm and hydrogen gas at a partial pressure of 0.229...
4. Now consider the catalase catalyzed decomposition of hydrogen peroxide to water. The much needed catalyst. 2H202 + catalase → 2H2O + O2 + catalase a. [3] Assume the following mechanism: H2O2 + catalase = {H202-catalase} HIS 54 Inhibitor ASN 127 H2O2 + {H202-catalase} → catalase + 2H20 + O2 Oxygen When the pre-equilibrium approximation is used, the rate-law is: 41 dt Kegk2[H202]?[E]. The steady-state approximation gives a more general rate law. Derive the rate law using the SS approximation....
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 + 0 + M 0+03 2 02 Apply the steady-state approximation to the concentration of atomic oxygen, and derive the rate law for the decomposition of ozone (M stands for a molecule that can exchange kinetic energy with particles undergoing the chemical reaction.)
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 +...
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...
Question 8 Step 1: H,02 + I +10- +H,0 Step 2: H,02 + 10 + H2O + O2 +I" The mechanism for a chemical reaction is shown above. Which of the following statements about the overall reaction and rate laws of the elementary reactions is correct? The chemical equation for the overall reaction is 2 H202 + I and the rate law for elementary step 2 is rate = k[H,02][10 + 2 H2O + O2 +I , ]. + H2O...
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'...
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
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