consider the overall reaction: AB(g) + CB(g) ⟶ A(g) + CB2(g) A proposed mechanism for this...
consider the overall reaction: AB(g) + CB(g) ⟶ A(g) + CB2(g)
A proposed mechanism for this reaction is
2 AB(g) ⇌ AB2(g) + A(g) (fast)
AB2(g) + CB(g) ⟶ AB(g) + CB2(g) (slow)
Based on this mechanism, determine the rate law for the overall reaction. Express your answer in terms of k and the necessary concentrations (ex: k[X][Y]^2). Use brackets around the concentrations and the caret symbol prior to the exponent. Do not include any multiplication signs. Type in subscripts as normal numbers (ex: AB2, CB2).
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consider the overall reaction: AB(g) + CB(g) ⟶ A(g) + CB2(g)
A proposed mechanism for this...
2 Rate = Consider the overall reaction: AB(g) + CB(g) ⟶ A(g) + CB2(g) A proposed...
2 Rate = Consider the overall reaction: AB(g) + CB(g) ⟶ A(g) + CB2(g) A proposed mechanism for this reaction is 2 AB(g) ⇌ AB2(g) + A(g) (fast) AB2(g) + CB(g) ⟶ AB(g) + CB2(g) (slow) Based on this mechanism, determine the rate law for the overall reaction. Express your answer in terms of k and the necessary concentrations (ex: k[X][Y]^2). Use brackets around the concentrations and the caret symbol prior to the exponent. Do not include any multiplication signs. Type...
Consider the overall reaction and proposed mechanism. step 1: A + BC --> AB + C...
Consider the overall reaction and proposed mechanism. step 1: A + BC --> AB + C step 2: AB + D --> AD + B step 3: B + C --> BC overall reaction: A + D --> AD What step is rate determining (slow) if the rate law of overall reaction is Rate = k[A][BC]
Part A Given the following proposed mechanism, predict the rate law for the overall reaction. 2...
Part A Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast Answer Choices: Rate =...
Consider the overall reaction and proposed mechanism. What step is rate determining (slow) if the rate...
Consider the overall reaction and proposed mechanism. What step is rate determining (slow) if the rate law of overall reaction is Rate = k[A][BC] step 1: A + BC --> AB + C step 2: AB + D --> AD + B step 3: B + C --> BC overall reaction: A + D --> AD
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step...
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....
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) →...
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? O k[no]/2[Hz] O k[N20][H2] O k[NO]2 O k[NO]2[Hz] O k[NO]2[H212
QUESTION 9 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1:...
QUESTION 9 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? k[N2O][H2] k[NO]2[H2] k[NO]2[H2]2 k[NO]1/2[H2] k[NO]2
QUESTION 19 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1:...
QUESTION 19 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO]1/2[H2] k[NO]2[H2] k[NO] [H2)2 k[N20][H2] k[NO]2
Ozone decomposes to molecular oxygen: 2 O3(g) ⇋ 3 O2(g). The following is a proposed mechanism...
Ozone decomposes to molecular oxygen: 2 O3(g) ⇋ 3 O2(g). The
following is a proposed mechanism for the reaction:
Step 1: O3(g) ⇋ O2(g) + O(g) (fast) Step 2: O3(g) + O(g) ⇋ 2
O2(g) (slow)
Provide a valid rate law for the overall ozone decomposition
reaction based on this mechanism.
4. Ozone decomposes to molecular oxygen: 203(g) — 3 O2(g). The following is a proposed mechanism for the reaction: Step 1: 03(g) – O2(g) + O(g) (fast) Step 2:...
A proposed mechanism for the reaction of NO_2 and CO is 2 NO_2(g) rightarrow NO(g) +...
A proposed mechanism for the reaction of NO_2 and CO is 2 NO_2(g) rightarrow NO(g) + NO_3(g) (Slow, endothermic) NO_3(g) + CO(g) rightarrow NO_2(g) + CO_2(g) (Fast, exothermic) a) Write the overall reaction. b) Identify each of the following as a reactant, product, , or intermediate, NO_2, CO, NO_3, CO_2, NO. c) Draw a reaction coordinate for this reaction. Indicate on this drawing the activation energy for each step and the overall enthalpy change. d) Give a plausible rate law.
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....
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? O k[no]/2[Hz] O k[N20][H2] O k[NO]2 O k[NO]2[Hz] O k[NO]2[H212
QUESTION 19 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO]1/2[H2] k[NO]2[H2] k[NO] [H2)2 k[N20][H2] k[NO]2
Ozone decomposes to molecular oxygen: 2 O3(g) ⇋ 3 O2(g). The
following is a proposed mechanism for the reaction:
Step 1: O3(g) ⇋ O2(g) + O(g) (fast) Step 2: O3(g) + O(g) ⇋ 2
O2(g) (slow)
Provide a valid rate law for the overall ozone decomposition
reaction based on this mechanism.
4. Ozone decomposes to molecular oxygen: 203(g) — 3 O2(g). The following is a proposed mechanism for the reaction: Step 1: 03(g) – O2(g) + O(g) (fast) Step 2:...
A proposed mechanism for the reaction of NO_2 and CO is 2 NO_2(g) rightarrow NO(g) + NO_3(g) (Slow, endothermic) NO_3(g) + CO(g) rightarrow NO_2(g) + CO_2(g) (Fast, exothermic) a) Write the overall reaction. b) Identify each of the following as a reactant, product, , or intermediate, NO_2, CO, NO_3, CO_2, NO. c) Draw a reaction coordinate for this reaction. Indicate on this drawing the activation energy for each step and the overall enthalpy change. d) Give a plausible rate law.
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