Part 1: Effect of Concentration The first part of the experiment is carried out at constant (room) temperature. Trial 1 is your baseline measurement. In Trials 2 and 3 you will change the concentration of Solution #1 or Solution #3, respectively.
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- 8 Reactions between certain organic (alkyl) halides and water produce alcohols. Consider the overall reaction for t-butyl bromide (2-bromo-2-methylpropane). (CH3)3CBr(aq) + H2O(1) →(CH3)3COH(aq) + H*(aq) + Br "(ag) k[(CH3)3CB1]. The accepted mechanism for the The experimental rate law is rate = %3D reaction is shown below. (1) (CH3)3C-Br(aq) →(CH3)3C*(aq) + Br "(aq) [slow] (2) (CH3)3C*(aq) + H2O(1) →(CH3)3C-OH2*(aq) [fast] (3) (CH3)3C-OH2*(aq) →H*(aq) + (CH3)3C-OH(aq) [fast] a) Why doesn't H2O appear in the rate law? b) Write rate laws for the elementary steps. c) What intermediates appear in the mechanism? d) Show that the mechanism is consistent with the experimental rate law. ed to the of consumption of NB. Concentration Table B: Reaction Rate of Na S O/HCI Beaker # 12345 A-Volume- of 0.15 M Na,S,O, (aq) used / ml. 50.0 40.0 30.0 20.0 10.0 B- Volume of water/mL. 0.0 10.0 20.0 30.0 40.0 Total volume (A+B) /ml 50.0 50,0 50.0 50.0 50.0 *Concentratio n of Na,8,0, (aq) /mol L 15 .12 090 060 030 Plot two graphs: 1. Time vs concentration of Na.S,O, (aq) 2. 1/Time vs concentration of Na S.O, (aq) Time/s 22.5 27.3 35.1 60.0 159.1 Explain the observations (relationship between concentration and time). 1/time/ 0444 0366 *Use civic₂V; to determine the concentration of the diluted sodium thiosulphate solution (beakers 2-5). On how to use this dilution formula, then, please watch: 0285 0167 00629Provide the products (or reactants) and the names of the reactions when needed. Fast pls i will give u like for sure solve this question correctly in 5 min pls
- Calibration Curve for the Kinetics Red Dye Lab You will be provided with a stock solution of Red Dye. From the information on the bottle, please calculate the molarity of the stock solution. Stock: 0.50|1 g of red dye per 100 mL of solution Show calculation for the molarity of stock solutionConsider chemical reaction:- X +2Y+ az )XY2Z2 It is faund that mng the [X] quadaup the [2] oubles the hate -) doubling the Cx7 has no effect on the sate doulbl les the late dneponb Cx] (- what is -the fate seaction 9 2 Pse dict the reactants for the Tate determ inA step. what is the molecularlty of the rate-deter step. minir 2) Predict a Complete mechanism Ahat meets the aiteria por this reaction Indicate which is neccessory the slow step the intermediates •J need these answer within 30 min. Thank Xou, Pleaze Consider g reguest my11) Explain fully using the collision theory. How the rate of reaction will change due to the partial evaporation of the solvent from the first reagent, before the addition of the second reagent? CCALE of 66001 Clas
- Final Reactant Concentrations and Reaction Rates [I-] [BrO3-] [H+] Reaction Time Rate of Reaction 2.8 x 10-5/time Expt. # M M M sec. M/sec 1 0.00166 0.0066 0.0166 258 3.876 x 10^-6 2 0.0033 0.0666 0.0166 135 7.40 x 10^-6 3 0.00166 0.0133 0.0166 132 7.576 x 10^-6 4 0.00166 0.0066 0.033 78 1.282 x 10^-5 Using the general rate law equation below and your orders determined, calculate the rate constant for each experiment and then the average. Rate= k[I-]m[BrO3-]n[H+]p k______________ k________________ k________________ k ____________ Average value of k __________________ Units of k__________________ Rewrite the final rate law including values for m, n, p and the average value of k and units: _________________________________A comparative analysis of organic compounds were done on various unknown samples labelled as A, G, N, U, Y. After multiple solubility tests, the following observations were recorded: I. Sample G dissolved in water and produced litmus paper results: Red → Red; Blue → Red II. Sample A did not dissolve in water, but dissolved in aq. HCl. III. Sample N did not dissolve in water, but dissolved in aq. NaOH. Further testing confirmed that it is insoluble in aq. NaHCO3. IV. Sample Y dissolved in water and produced litmus paper results: Red → Blue; Blue → Blue V. Sample U is insoluble in H2O, aq. NaOH, aq. HCl and concentrated H2SO4. What is the most probable identity of sample G? What is the most probable identity of sample A? What is the most probable identity…A comparative analysis of organic compounds were done on various unknown samples labelled as A, G, N, U, Y. After multiple solubility tests, the following observations were recorded: I. Sample G dissolved in water and produced litmus paper results: Red → Red; Blue → Red II. Sample A did not dissolve in water, but dissolved in aq. HCl. III. Sample N did not dissolve in water, but dissolved in aq. NaOH. Further testing confirmed that it is insoluble in aq. NaHCO3. IV. Sample Y dissolved in water and produced litmus paper results: Red → Blue; Blue → Blue V. Sample U is insoluble in H2O, aq. NaOH, aq. HCl and concentrated H2SO4. What is the most probable identity of sample G? What is the most probable identity of sample A? What is the most probable identity…
- In the reaction X(p, a) PC, Xis. O N o o No O "NFor the reversible, one-step reaction A + A * k_{1}/k_{-1} * B + C the rate constant for the forward reaction, k_{1} , is 279 L* mol^ -1 * min^ -1 and the rate constant for the reverse reaction, k_{1} is 355Lmo * l ^ - 1 * mi * n ^ - 1 at a given temperature . The activation energy for the forward reaction is 43.3kJmo * l ^ - 1 whereas the activation energy for the reverse reaction is 22.8kJmo * l ^ - 1Determine the equilibrium constant, K, of this reaction.At 40^0c, H202 (aq) will decompose according to the foll. reaction: 2 H202 (aq) ----2H20(l) +02 (g) The foll. data were collected for the concentration of h202 at various times. Time. [H202] (mol/L) 0. 1.600 3.10*10^4 0.592 6.20*10^4. 0.219 (a) Calculate the average rate of decomposition in H202 between0 and 3.10 * 10^4 s. use this rate to calculate the average rate of production 02 (g) over the same time period. (b) What are these rates for the time period 3.10*10^4 s. to 6.20 *10^4 s.? Rate of H202 decomposition Rate of O2 Production