5. Iodide is oxidized by hydrogen peroxide according to the following mechanism: H 2 O 2...
5. Iodide is oxidized by hydrogen peroxide according to the following mechanism:
H 2 O 2 + I- → H 2 O + OI- (slow)
H+ + OI- → HOI (fast)
HOI + H+ + I- → I2 + H2O (fast)
(a) What is the overall reaction?
(b) What is the molecularity of each step?
(c) Write the rate equation for the rate-determining step.
(d) What are the intermediates in this reaction? (If none, write “none.”)
Homework Answers
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5. Iodide is oxidized by hydrogen peroxide according to the
following mechanism:
H 2 O 2...
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5. Carcinogenic nitrosamines are produed from amines such as dimethylamine and nitrous acid according to the following mechanism: H + + HNO 2 → H 2 NO 2 + (fast, reversible) H 2 NO 2 + + (CH 3 ) 2 NH → (CH 3 ) 2 NHNO + + H 2 O (slow) (CH 3 ) 2 NHNO + → (CH 3 ) 2 NNO + H + (fast) (a) What is the overall reaction? (b) What is the...
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#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2 2Br fast Step 2 Br + H2 H2Br fast Step 3 H2Br + Br 2HBr slow a. What is the overall equation? b. Identify the intermediate(s) if any. c. What is the molecularity and the rate law for each step including any reversible steps? d. What is the predicted rate law expression for this reaction. Be sure to only list reactants from the overall equation and...
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 ...
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II. Show your work in detail (step by step). You must show your work. The following mechanism has been suggested for the reaction: H2O2 + 2H+ + 2I – ® I2 + 2H2O H2O2 + I – ® HOI + OH – Slow OH – + H+ ® H2O Fast HOI + H+ + I – ® I2 + H2O Fast Identify all intermediates included in this mechanism.
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2 H2O2(aq) + 2 H2O(l) + O2(g) 5. Hydrogen peroxide decomposes according to the equation above. a. An aqueous solution of H2O, that is 6.00 percent H,O, by mass has a density of 1.03 g ml. Calculate each of the following. (i) The original number of moles of H2O, in a 125 ml sample of the 6.00 percent H2O2 solution (ii) The number of moles of O,(g) that are produced when all of the H2O2 in the 125 mL sample...
Help Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous...
Help Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution H + H202H20' -ΟΗ (rapid equilibrium) H20 -OH + Br - HOBr + H20 (slow) HOBr + Η* - Βr - Βι2 + H20 (fast) What is the overall reaction equation for this process? 0005 Multiple Choice -Book Ο None of these choices are correct Ο H2O-OH + B H Br2 + H20 Ο 2Η Η2Ο2 Β- MO H2OOH - B2 H2O...
The reaction between peroxide (H2O2) and iodide in basic solution is proposed to occur according to...
The reaction between peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\) and iodide in basic solution is proposed to occur according to the following mechanism:Step \(1: \mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{I}^{-} \rightarrow \mathrm{HOl}+\mathrm{OH}^{-}\) slowStep \(2: \mathrm{OH}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{H}_{2} \mathrm{O}\) fastStep \(3: \mathrm{HOl}+\mathrm{H}^{+}+\mathrm{I}^{-} \rightarrow \mathrm{I}_{2}+\mathrm{H}_{2} \mathrm{O}\) fastThe rate law for this mechanism would be?Select one:O. Rate \(=\mathrm{k}\left[\mathrm{H}_{2} \mathrm{O}_{2}\right][\mathrm{I}]\left[\mathrm{OH}^{-}\right]\left[\mathrm{H}^{+}\right]\)0. Rate \(=k\left[\mathrm{H}_{2} \mathrm{O}_{2}\right]\)O C. Rate \(=k[\mathrm{OH}]\left[\mathrm{H}^{+}\right]\)O d. Rate \(=k\)O e. Rate \(=\mathrm{k}\left[\mathrm{H}_{2} \mathrm{O}_{2}\right][\mathrm{I}]\)
Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid...
Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H202 = H207-OH (rapid equilibrium) H207-OH + Br- → HOBr + H20 (slow) HOBr + H+ + Br + Br2 + H20 (fast) What is the overall rate of reaction?
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
The following mechanism, proposed for the decomposition of hydrogen peroxide is composed of 2 elementary steps:...
The following mechanism, proposed for the decomposition of hydrogen peroxide is composed of 2 elementary steps: H2O2(aq) + I'(aq) > H2O(l) + 10 (aq) 10 (aq) + H2O2(aq) -> H2O(l) + O2(g) + I'(aq) The rate law predicted by the mechanism is slow fast a) rate = k [H2O2) b) rate =k [H202][I] c) rate =k [H2O2][10] d) rate = k [H202) [1]
2 H2O2(aq) + 2 H2O(l) + O2(g) 5. Hydrogen peroxide decomposes according to the equation above. a. An aqueous solution of H2O, that is 6.00 percent H,O, by mass has a density of 1.03 g ml. Calculate each of the following. (i) The original number of moles of H2O, in a 125 ml sample of the 6.00 percent H2O2 solution (ii) The number of moles of O,(g) that are produced when all of the H2O2 in the 125 mL sample...
Help Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution H + H202H20' -ΟΗ (rapid equilibrium) H20 -OH + Br - HOBr + H20 (slow) HOBr + Η* - Βr - Βι2 + H20 (fast) What is the overall reaction equation for this process? 0005 Multiple Choice -Book Ο None of these choices are correct Ο H2O-OH + B H Br2 + H20 Ο 2Η Η2Ο2 Β- MO H2OOH - B2 H2O...
The reaction between peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\) and iodide in basic solution is proposed to occur according to the following mechanism:Step \(1: \mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{I}^{-} \rightarrow \mathrm{HOl}+\mathrm{OH}^{-}\) slowStep \(2: \mathrm{OH}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{H}_{2} \mathrm{O}\) fastStep \(3: \mathrm{HOl}+\mathrm{H}^{+}+\mathrm{I}^{-} \rightarrow \mathrm{I}_{2}+\mathrm{H}_{2} \mathrm{O}\) fastThe rate law for this mechanism would be?Select one:O. Rate \(=\mathrm{k}\left[\mathrm{H}_{2} \mathrm{O}_{2}\right][\mathrm{I}]\left[\mathrm{OH}^{-}\right]\left[\mathrm{H}^{+}\right]\)0. Rate \(=k\left[\mathrm{H}_{2} \mathrm{O}_{2}\right]\)O C. Rate \(=k[\mathrm{OH}]\left[\mathrm{H}^{+}\right]\)O d. Rate \(=k\)O e. Rate \(=\mathrm{k}\left[\mathrm{H}_{2} \mathrm{O}_{2}\right][\mathrm{I}]\)
Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H202 = H207-OH (rapid equilibrium) H207-OH + Br- → HOBr + H20 (slow) HOBr + H+ + Br + Br2 + H20 (fast) What is the overall rate of reaction?
The following mechanism, proposed for the decomposition of hydrogen peroxide is composed of 2 elementary steps: H2O2(aq) + I'(aq) > H2O(l) + 10 (aq) 10 (aq) + H2O2(aq) -> H2O(l) + O2(g) + I'(aq) The rate law predicted by the mechanism is slow fast a) rate = k [H2O2) b) rate =k [H202][I] c) rate =k [H2O2][10] d) rate = k [H202) [1]
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