Homework Answers
Step (1): NO2+
F2 ------> NO2F + F Rate (1): k1[NO2][F2]
Step (2): NO2 + F -------> NO2F Rate (2): k2[NO2][F]
Overall Reaction: 2 NO2 + F2 ---------> 2NO2F
Step (1) and (2) add up to an overall reaction that matches the stoichiometry of the given equation. The rate of Step (2) is consistent with the experimental rate law. Therefore, the proposed mechanism works. The slowest elementary process gives the rate of the overall reaction. Since the rate of Step (2) matches the experimental rate law, Step (2) is the rate determinant. Step (1) has a faster reaction.
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03 (5 marks) : propose a two-step (elementary) mechanism for the reaction: 2NO2(g) + F2(g) →...
The reaction 2NO2(g)+F2(g)→2NO2F(g) has a second order rate law, rate=k[NO2][F2]. Suggest a mechanism that is consistent...
The reaction 2NO2(g)+F2(g)→2NO2F(g) has a second order rate law, rate=k[NO2][F2]. Suggest a mechanism that is consistent with this rate law.
6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g)...
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Consider the recombination reaction: 2 Br(g) Br2 (8) The mechanism involves two elementary steps. The first...
Consider the recombination reaction: 2 Br(g) Br2 (8) The mechanism involves two elementary steps. The first step results in formation of an energized Bra molecule, the excess energy carried by Bris then transferred to a molecule M for subsequent formation of Bry in the second step First step: 2 Br (8) Bry* () + M ) Brz* () Brz () +M() Second step: By the steady-state approximation and work out an expression for d[Brydr in term of k, k., ky...
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A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step...
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step by step
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1. Write a rate law from the image below: TRANSITION STATES Ea(step 2) Ea(step 1) slow...
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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...
6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g) The mechanism proposed for this reaction is as follows: (i) NO2(g) + F2(g) → NO2F(g) + F(g) (ii) NO2(g) + F(g) → NO2F(g) Which elementary step is the rate-determining step in this reaction? Explain your answer in 1-2 sentences.
Consider the recombination reaction: 2 Br(g) Br2 (8) The mechanism involves two elementary steps. The first step results in formation of an energized Bra molecule, the excess energy carried by Bris then transferred to a molecule M for subsequent formation of Bry in the second step First step: 2 Br (8) Bry* () + M ) Brz* () Brz () +M() Second step: By the steady-state approximation and work out an expression for d[Brydr in term of k, k., ky...
Propose a plausible two-step mechanism for the given reaction (Pool: 5 of 5) Propose a plausible two-step mechanism for the reaction given below with the steps provided. Overall Reaction: 2A + 2B rightarrow C + D Experimentally Determined Rate Law: rate = K[A][B]^2 Two-Step Mechanism: Step 1: Step 2:
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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....
step by step
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