Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1 Step 2: NO(g) + )...
Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1
Step 2: NO(g) + ) --> NO2 (g) rate = k2
suppose that k1<<k2, That is the first step is much slower than the second.
Write the balanced chem equation for the overall chemical rxn
Write the experimentally observable rate law for the overall reaction. (no reaction concentrations) rate=k()
Express the rate constant k for the overall reaction in terms of k1, k2 and (if necessary) the rate constant k_1 and k_2 for the reverse of the 2 elementary reactions in the . mechanism. k= ()
Homework Answers
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Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1
Step 2: NO(g) + )...
Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: rate constant elementary...
Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: rate constant elementary reaction step NO(g)+ 02(g) NO2(9) 0(g) 1 NO(g) O(g) NO2(9) k2 2 Suppose also k,»k,. That is, the first step is much faster than the second. 2* Write the balanced chemical equation for the overall chemical reaction: Write the experimentally observable rate law for the overall chemical reaction rate k Note: your answer should not contain the concentrations of any intermediates. Express the rate...
— O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism Suppose the...
— O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism Suppose the formation of nitrosyl chloride proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + Cl2(9) ► NOCI (9) km 2 NOCI (9) + NO(g) → 2 NOCI (9) kz Suppose also k«k. That is, the first slower than the second 0-0 Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical...
Can check my answrs as well if it's correct and help me out with the last...
Can check my answrs as well if it's correct and help me out with
the last part of the question.
Suppose the decomposition of dinitrogen monoxide proceeds by the following mechanism: step elementary reaction rate constant ki N2O(g) → N2(9) + O(g) 2 N2O(g) + 0(g) N2(g) + O2(9) k Suppose also k,«k2. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: 2N 0(3) 2N, (g) + 02...
Suppose the synthesis of ethylene dichloride proceeds by the following mechanism: step rate constant elementary reaction...
Suppose the synthesis of ethylene dichloride proceeds by the following mechanism: step rate constant elementary reaction CH,CH, (g)+ci, (g) → CH,CH,ci* (g)+ciº (9) CH,CH,CI* (g)+C1 (g) → CH,CH,C1, (g) Suppose also kq «k2. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. rate = % 0
step Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: elementary reaction...
step Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: elementary reaction rate constant NO(g) +0,() ► NO,()+(2) ky 2 NO(g) +0 (2) NOG) kz Suppose also , ekz. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates x 5 ?
Step 1: 03 (g) + NO (g) = NO2 (g) + O2 (g) Step 2: NO2...
Step 1: 03 (g) + NO (g) = NO2 (g) + O2 (g) Step 2: NO2 (g) + O (9) NO (g) + O2 (g) PE "IM Reaction path What is the overall rate law? Rate = k[O3] Rate = k[O3][0] Rate = k[O3][NO]
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....
Consider the following chemical reaction, at 500degree C and 200atm, for question 1-5: Step1: NO_2(g) +...
Consider the following chemical reaction, at 500degree C and 200atm, for question 1-5: Step1: NO_2(g) + F_2(g) rightarrow NO_2F(g) + F(g) Step 2: NO_2(g) + F_2(g) rightarrow NO_2F(g) rate determining step After this two-step process occurs, what is the overall balanced chemical equation? NO_2(g) + F_2(g) rightarrow NO_2F(g) + F(g) NO_2(g) + F_2(g) rightarrow NO_2F(g) + F_2(g) 2NO_2(g) + F_2(g) rightarrow 2NO_2F(g) 2NO_2(g) + F_(g) rightarrow 4NO_(g) + F(g) What is the intermediate this multistep mechanism? NO_2(g) F_(g) NO_2F_(g) F_2(g)...
ki Q3: The decomposition mechanism of 2 N2O(g) → 4NO2(g) + O2(g) is believed to follow...
ki Q3: The decomposition mechanism of 2 N2O(g) → 4NO2(g) + O2(g) is believed to follow the elementary reactions: (1) N203 → NO2 + NO3 (1') NO2 + NO3 → N20 k_1 (2) NO, + NO3 → NO, + O2 + NO kz (3) NO + N203 → NO2 + NO2 + NO2 kz Using the steady-state approximation, deduce the rate law for this reaction.
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 ...
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...
Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: rate constant elementary reaction step NO(g)+ 02(g) NO2(9) 0(g) 1 NO(g) O(g) NO2(9) k2 2 Suppose also k,»k,. That is, the first step is much faster than the second. 2* Write the balanced chemical equation for the overall chemical reaction: Write the experimentally observable rate law for the overall chemical reaction rate k Note: your answer should not contain the concentrations of any intermediates. Express the rate...
— O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism Suppose the formation of nitrosyl chloride proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + Cl2(9) ► NOCI (9) km 2 NOCI (9) + NO(g) → 2 NOCI (9) kz Suppose also k«k. That is, the first slower than the second 0-0 Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical...
Can check my answrs as well if it's correct and help me out with
the last part of the question.
Suppose the decomposition of dinitrogen monoxide proceeds by the following mechanism: step elementary reaction rate constant ki N2O(g) → N2(9) + O(g) 2 N2O(g) + 0(g) N2(g) + O2(9) k Suppose also k,«k2. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: 2N 0(3) 2N, (g) + 02...
Suppose the synthesis of ethylene dichloride proceeds by the following mechanism: step rate constant elementary reaction CH,CH, (g)+ci, (g) → CH,CH,ci* (g)+ciº (9) CH,CH,CI* (g)+C1 (g) → CH,CH,C1, (g) Suppose also kq «k2. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. rate = % 0
step Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: elementary reaction rate constant NO(g) +0,() ► NO,()+(2) ky 2 NO(g) +0 (2) NOG) kz Suppose also , ekz. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates x 5 ?
Step 1: 03 (g) + NO (g) = NO2 (g) + O2 (g) Step 2: NO2 (g) + O (9) NO (g) + O2 (g) PE "IM Reaction path What is the overall rate law? Rate = k[O3] Rate = k[O3][0] Rate = k[O3][NO]
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....
Consider the following chemical reaction, at 500degree C and 200atm, for question 1-5: Step1: NO_2(g) + F_2(g) rightarrow NO_2F(g) + F(g) Step 2: NO_2(g) + F_2(g) rightarrow NO_2F(g) rate determining step After this two-step process occurs, what is the overall balanced chemical equation? NO_2(g) + F_2(g) rightarrow NO_2F(g) + F(g) NO_2(g) + F_2(g) rightarrow NO_2F(g) + F_2(g) 2NO_2(g) + F_2(g) rightarrow 2NO_2F(g) 2NO_2(g) + F_(g) rightarrow 4NO_(g) + F(g) What is the intermediate this multistep mechanism? NO_2(g) F_(g) NO_2F_(g) F_2(g)...
ki Q3: The decomposition mechanism of 2 N2O(g) → 4NO2(g) + O2(g) is believed to follow the elementary reactions: (1) N203 → NO2 + NO3 (1') NO2 + NO3 → N20 k_1 (2) NO, + NO3 → NO, + O2 + NO kz (3) NO + N203 → NO2 + NO2 + NO2 kz Using the steady-state approximation, deduce the rate law for this reaction.
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