Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. Elementary Step 1 H+ + H₂O₂ = {H₂O*- OH) (rapid equilibrium) Elementary Step 2 (H₂O+-OH) + Br¯ → HOBr + H₂O (slowest) Elementary Step 3 HOBr + H+ + Br¯ → Br₂ + H₂O (fast) Consider the reaction profile below. Approximate the AH for elementary step 2 only?

Q: The second-order rate constant for the following gas-phase reaction is 0.043 1/M-s. We start with…

A: Given: The rate constant of the second-order reaction is 0.0431 M-1 s-1. The number of moles of C2F4…

Q: 0.065 10 0.0625 20 0.06 2 NH3 (g) → N2 (g) + 3 H2 (g) at 1100 degrees C 30 0.0575 40 0.055 50 0.0525…

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A: We have given that  2NO + Br2 → 2NOBr    NO + Br2  ⇌K-1K1  NOBr2  ( fast equilibrium )   NOBr2  + NO…

Q: Consider the reaction 2H3PO4→P2O5+3H2O Using the information in the following table, calculate the…

A: The reaction is 2H3PO4⟶P2O5+3H2O  Rate of reaction =-12ΔH3PO4Δt=ΔP2O5Δt=13ΔH2OΔt

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Q: The second-order rate constant for the following gas-phase reaction is 0.042 1/M.s. We start with…

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Q: Consider the mechanism. Step 1: Step 2: E Overall: A+ D B+E Determine the rate law for the overall…

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Q: The reaction between selenious acid and iodide ion in acid solution is H2SeO3 + 6I- + 4H+ ⇌ Se +…

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Q: A chemistry graduate student is studying the rate of this reaction: NH,OH(aq) - NH, (aq)+H,O(aq) He…

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Q: What is the intermediate for the reaction based on the proposed mechanism shown below? 2 NO2(g) +…

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Q: Write the balanced overall reaction for the three-step mechanism. 1. C₂H, Br C₂H+ Br 2. C₂H+H₂O →…

A: Reaction : 1. C4H9Br →C4H9++Br- 2. C4H9++H2O →C4H9OH2+ 3.C4H9OH2++H2O →C4H9OH + H3O+

Q: What is the rate constant of a first-order reaction when 20.0% of a reactant remains after 30.0 s?

A: This is first order reaction.For first order reaction, rate law is

Q: In Figure 14.3, order the following three rates from fastest to slowest: (i) The averagerate of the…

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Q: The second-order rate constant for the following gas-phase reaction is 0.04 1/M.s. We start with…

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Q: 2H2O2---> 2H2O+ O2 Calculate the instantaneous rate of formation of O2 at 50 seconds.

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Q: Based on the provide elementary steps below, determine the net reaction. NO,CI (g) – NO2 (g) + CI…

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Q: Consider the mechanism. Step 1: A+B Step 2: A+ C Overall: 2 A+B D Determine the rate law for the…

A: Answer :--  Given :--  Step 1:        A + B ---> C     slow  Step 2:        A + C ---> D…

Q: The rate constant for the second order reaction 2 NO2  2 NO + O2 is 0.31 M-1s-1.  If a 4.33 M sample…

A: In order to calculate the concentration of nitrogen dioxide we first write down the given data:…

Q: Analyze the following mechanism: What are the intermediates and catalysts if there are any? What is…

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Q: For the first-order reaction, 2N₂O(g) → 2N2(g) + O2(g), what is the concentration of N₂O after 3…

A: we have to determine the final concentration of N2O

Q: For the following reaction, to get the rate of formation of H2O, what must we multiply the rate of…

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Q: In a first-order reaction where A is the reactant and k = 0.0150 min 1. If [A] is 0.400 M initially,…

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Q: The reaction: A + 3B-> D + F was studied and the following mechanism was determined A+ B-> C (fast)…

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Q: At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.0162…

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Q: Consider the reaction below. The reaction starts with an initial concentration [A] of 3.50x10-2 M…

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Q: At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.0618…

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Q: The graphs below show sample data for reactant A. All the other reactants are in excess. Identify…

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