Iodination of Acetone

Draw the mechanism of the reaction.

The following initial rate data are for the reaction of tertiary butyl bromide with hydroxide ion at 55 °C: (CH3)3CB + OH → (CH3)3COH + Br Experiment [(CH3)3CB1],, M [OH], M Initial Rate, Ms-1 1 0.890 1.50x10-3 1.50x10-3 3.01x10-3 3.01x10-3 0.118 0.118 2 1.78 0.890 1.78 3 0.237 4 0.237 Complete the rate law for this reaction in the box below. Use the form k[A]j™[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is

What is the full mechanism of this reaction?

1 The rate of reaction between butanone and iodine is studied. In this experiment, iodine is in excess. The concentration of butanone is measured at various time intervals. The results are shown in the table below. Time / min 10 20 30 40 50 60 80 100 120 [butanone] / 0.080 0.055 0.035 0.024 0.015 0.010 0.007 0.003 0.001 0.001 moldm Chapter 22: Reacti a Plot these data on a suitable graph. b Show from your graph that these data are consistent with the reaction being first order with respect to butanone. C Find the gradient of your graph when the butanone concentration is: 1 0.070 mol dm 1 0.040moldm3 1 0.010mol dm

Show detailed reaction mechanisms for the following reaction. Include all relevant resonance structures and the structure of the expected organic and inorganic products.

Although you may not have seen the reaction highlighted in green before, it uses similar chemical concepts you have seen in other reaction mechanisms. Draw the mechanism.

estion 8 (2 points) E Listen Given the reaction: (CH3)3CCI + OH* ----> (CH3)3COH + Cl, it has experimentally found that doubling the concentration of (CH3)3CCI causes the reaction rate to be increased twofold, but doubling the concentration of OH- has no effect on the rate. The final rate law equation, expressed mathematically is: R = k [(CH3)3CCI] [OH-] R = k [(CH3)3CCI] R = k [(CH3)3CCI]2 [OH-] R = k [(CH3)3COH] [CI-] OR= k{[(CH3)3COH][CI-] / [CH3)3CCI][OH-]}

The below reaction follows second order rate kinetics and proceeds via a bimolecular mechanism. KCNCH3B1 -» KBr + CH3CN If the concentration of potassium bromide were doubled, how many times faster would the reaction go? If the concentration of CH3Br were doubled. How much faster would the reaction go? Write the rate law for the above reaction. If [KCN] 0.5 M, [CH3Br] 0.5 M, and the relative reaction rate is 0.25 M/s, what is the rate constant? Also, what are the units of the rate constant?

The activation energy for the gas phase decomposition of cyclobutane is 262 kJ. (CH₂) 4- →2 C₂H4 The rate constant at 721 K is 0.000401 /s. The rate constant will be 0.00338/s at K.

Experimental Procedure, Part F. A 1.0 mL volume of .010 M H2SO3 is added to a mixture of 6 drops of .010 M HIO3, 14 drops of deionized water, and 1 drop of starch solution. A color change in the reaction mixture occurred after 56 seconds. The rate of the reaction is measured by the disappearance of HIO3. For the reaction mixture in this question, what is the reaction rate? Express the reaction rate in units of mol HIO3/L/sec to the correct number of significant figures.?

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)

Draw a mechanism for the following intramolecular Mizoroki-Heck reaction. The Pd catalyst can be abbreviated as [Pd]. Br Me Pd(PPH3)4 (5 mol%) Et3N DMF, 90°C Me

The following molecule has been formed by combining ketone and KCN (cyanohydrin) Sketch a skeletal formula for this reaction and using the curly arrow notation, give the reaction mechanism for this reaction.

Sagr.0909

19. 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 so onNote for advanced students: you may assume these reactions all take place in a polar aprotic solvent, like DMSO.

please help me answer a & b

2.) The reaction between acetone (CH3COCH3) and bromine in acid solution was studied and the following rate data collected. Determine the rate law by calculating the reaction orders with respect to each reactant and the value for the rate constant, k. Show ALL work. [Acetone] [Br2] [H3O*] (M) Rate Trial (mol*L·l*s•l) 5.8 x 10-5 5.8 x 10-5 (M) (M) 0.30 0.050 0.050 0.30 0.100 0.050 1.2 x 104 3.2 x 10-4 3 0.30 0.050 0.100 4 0.40 0.050 0.200

Do you agree or disagree with this proposed mechanism? Explain.

Answer all multiple choice questions please

Calculate the time (min)required for a first-order reaction A -> Product to be 64.9% completed, knowing that the half lifetime t 1/2 is 206 min

Based on the time and temperature data collected for the reaction of KMnO4 with either malonic acid or oxalic acid, one can conclude that generally as the temperature of a reaction is increased, the rate of the reaction increases. This is because, the activation energy is lowered and the reactant molecules collide with greater energy the activation energy is lowered and the reactant molecules collide more frequently the activation energy is lowered, the reactant molecules collide more frequently and with greater energy per collision O the reactant molecules collide more frequently and with greater energy per collision

Hydrogen gas reduces NO to N2 in the following reaction: 2H, (g) + 2NO(g) 2H,0(g) +N, (g) The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2]o (M) [NO]o (M) Initial Rate (M/s) 1 0.212 0.136 0.0393 0.212 0.272 0.0789 3 0.424 0.544 0.624 4 0.848 0.544 2.50

When fitting data to a best fit line, a correlation coefficient (R2) is determined and used to evaluate the quality of fit. The best fit of the data will have an R² value closest or equal to zero (0). closest or equal to one (1). equal to the rate of the reaction occurring. equal to the rate constant of the reaction occurring.

Which of these two reactions has a faster rate and why

Consider the energy diagram for the reaction A -> B. Identify the intermediate, the transition state, and the activation energy for this reaction.

Please show your work (this is not a graded assignment)

Consider the following elimination reaction:   Use the following data to identify the rate-determining step of the above reaction. Justify your rate law and overall reaction order based on this mechanistic step Experiment [Alcohol] [H+] Rate (M/s) 1 1.00 1.00 1.6 x 10-6 2 2.00 1.00 3.2 x 10-6 3 1.00 2.00 1.6 x 10-6 Knowing the overall reaction order, calculate the rate constant and the half-life of this reaction.

What is the half-life for a 2nd order reaction (const. temp. & P): A > B whose initial concentration is 0.500 M, with a k = 6.28 x 10-3 M-' 517 What is the rate constant (in s-') for a 1st order reaction (const. temp. & P): A > B having a starting concentration of 1.50 M, with a half-life of 3.88 minutes? 60 s = 1 min. For the reaction at const. temp.: A > B, having k = 2.26 x 103 M's', how long would it take, IN MINUTES, for [A] to decline to 0.286 M when [A] =1.00 M?