Predict the relative rates of these reactions. That is, select 1 next to the reaction with the fastest rate, 2 next to the reaction with the next fastest rate, and soon.Note for advanced students: you may assume these reactions all take place in a polar aprotic solvent, like DMSO.OH2+ ciReactionRelative RateХ(Choose one)+ H2OOH2F(Choose one)+ F+ H₂OOH2OH2+BrBr(Choose one)+ H2O(Choose one)+ H₂OG

Step 1:The reactant in all the reactions is protonated alcohol (H2O+ is the leaving group) and the…

Answered: Predict the relative rates of these…

Organic Chemistry: A Guided Inquiry

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Chapter13: Substitution

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propan-1-ol → propene + water C₃H₈O (l) → C3H6 (g) + H2O (l) is considered an Elimination E2 reaction. An E2 Elimination is apparently where an external base is added, so the rate law should be rate = k[C₃H₈O][Base] however the rate law I have is only = k[C₃H₈O]. However, in this reaction, it seems no bases are involved because the catalyst being used is sulfuric acid, which is definitely not a base. Can someone help me with what I am missing here? What factors affect the rate of E2 elimination? Some say that one factor is a strong attacking base -- which I do not think I have. Please help!! I am so very lost
(a) Select all of the correct statements about reaction rates from the choices below. The lower the rate of a reaction the longer it takes to reach completion. A balanced chemical reaction is necessary to relate the rate of reaction to the concentration of a reactant. As a reaction progresses its rate goes down. The rate of a slow step has more effect on the overall reaction rate than the rate of a fast step. Reaction rates are determined by reactant concentrations, temperatures, and reactant stabilities. Reaction rates increase with increasing temperature. Reactions involving very unstable combinations of chemicals have large rate constants.
Order the following organic reactions by relative rate. That is, select '1' next to the reaction that will have the fastest initial rate, select '2' next to the reaction that will have the next fastest initial rate, and so on. If two reactions will have very similar initial rates, you can select the same number next to both. If a reaction will have zero or nearly zero initial rate, don't select a number and check the box in the table instead. Note: the "Nu" in these reactions means "a generic nucleophile." ملی CI :Nu 2 он 3 H Reaction Relative Rate (Choose one) ▼ Nu :CI: zero or nearly zero Nu :Nu bi (Choose one) zero or nearly zero : Nu لی Nu :H (Choose one) zero or nearly zero
Consider the below reaction mechanism:Step 1: S(s) + O2(g) SO2(g) fast; k1 = rate constant for forward reaction; k-1 = rate constant for reverse reactionFileStep 2: SO2(g) + 1/2 O2(g) SO3(g) slow; k2 = rate constantFileStep 3: SO3(g) + H2O(l) H2SO4(l) fast, k3 = rate constant a) Write the overall reactionb) Identify the intermediaries, if any.c) What is the rate law of the overall reaction?
16. Step 1 Step 2 Step 3 Students in a SCH4U class were examining the reaction between 2-bromo-2-methlypropane and water: (CH3)3CBr (aq) + H₂O (1)→ (CH3)3COH (aq) +H* (aq) + Br (aq) Their rate experiments show that the reaction is first order in (CH3)3CBr, but zero order in water. One of the students, Yuek-Fen, presented the following rate mechanism to her class for the above reaction. Determine if the mechanism below is plausible. Explain how you arrived at your decision. (CH3)3CBr (aq) → (CH3)3C (aq) + Br(aq) (CH3)3CH (aq) + H₂O (1)→ (CH3)3COH₂¹ (29) (fast) (CH3)3COH₂+ (aq) → 2H+ (aq) + (CH3)3COH (aq) Is this mechanism plausible? Explanation: (yes or no) (slow) (fast)
Real Time uy 12. A particular reaction requires 54 kJ mol to activate and is found to have a rate constant 1 -1 -1 -1 S S of 3.42 x 10-4 M¹s¹ at 155.85 °C. Predict the rate constant (in M¹ s¹ to two decimal places) if the temperature was increased to 460.85 °C. Approximately how much faster (to the nearest whole number) is the reaction predicted at 460.85 °C relative to 155.85 °C? A: 540 times faster
Chemistry (2023) 1 (iii)
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rate expression: rate = k[H2O2]m[I-]n 1. Would your specific rate constant, k, be larger than, smaller than, or unchanged from the correct value as a result of each of the following mistakes? Justify your answers. a) You accidentally substituted a value for n twice as great as it should have been when calculating k. b) Your water bath in the 600-mL beaker was about 5ºC warmer than room temperature for all three of your experiments.
The overall reaction #5 is referencing is above (first image). I DO NOT need help with #4, just #5, but 5D has to do with 4. I'm looking for some help with my main part of my question, number 5 A-D, but part 5D also asks for enthalpy values (I guess calculated from my first image)? I think the reaction is second order, but I'm not sure - I think it's second order because of the units Lmol^-1s^-1? And I don't really understand how to sketch a reaction energy diagram...
(a) Select all of the correct statements about reaction rates from the choices below. The lower the rate of a reaction the longer it takes to reach completion.Reactions involving very unstable combinations of chemicals have large rate constants.Concentrations of homogeneous catalysts have no effect on reaction rates.Reaction rate constants are independent of temperature.The slowest step in a reaction is called the rate-determining step.A balanced chemical reaction is necessary to relate the rate of reaction to the concentration of a reactant.Slow reactions can be speeded up by raising the temperature.
The data below show the concentration of N2O5 versus time for the following reaction: N2O5 (g) → NO3 (g) + NO2(g) Time (s) [N2O5] (M) 1.000 25 0.822 50 0.677 75 0.557 100 0.458 125 0.377 150 0.310 175 0.255 200 0.210

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