Vilsmeier Reactionمین الرسم اCHO----في ومنه استخدمPOCIDMFVILSMEIERCHO

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Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 55E: Describe how graphical methods can be used to determine the activation energy of a reaction from a...

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Similar questions

Determine the ΔSsystem given the reaction. C6H12O6(s) + O2(g) ----> CO2(g) + H2O(l).
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
Describe how graphical methods can be used to determine the activation energy of a reaction from a series of data that includes the rate of reaction at varying temperatures.
6 I- + BrO3- + 6 H+ ----- 3 I2 + Br- + 3 H2O Rate= k[I-]m[BrO3-]n[H+]p rate= (∆[I2])/(3*∆time) Trial [I-] (M) [BrO3-] (M) [H+] (M) 1 1.67*10-3 6.67*10-3 1.67*10-2 2 3.33*10-3 6.67*10-3 1.67*10-2 3 1.67*10-3 1.33*10-2 1.67*10-2 4 1.67*10-3 6.67*10-3 3.33*10-2 Reaction time: Trial 1 - 301.90 secs Trial 2 - 213.28 secs Trial 3 - 214.92 secs Trial 4 - 86.45 secs Calculate the rate for each trial and Using the information above determine the rate law (m, n and p) for the reaction. m_____________ n_________________ p ____________ Rate= k[I-]m[BrO3-]n[H+]p
Find DG° for this reaction: CH4 (g) + 2O2(g)+ ---> CO2 (g)+ 2H2O (l) Substance DGfdegree (kJ/mol) CH4(g) -50.66 O2(g) 0 CO2(g) -394.4 H2O(l) -237.4 A –682.5 kJ B 131.1 kJ C –581.1 kJ D -919.9 kJ E -818.5 kJ
Predict the products the reactions, if there is none, write NO RXN. Also indicate, if the reaction isfast or slow.
The ha lf-l ife of pyruvic acid in the presence of an aminotransferaseenzyme (which converts it to alanine) was found to be 221 s. How long will it take for the concentration of pyruvic acid to fal l to 1/ 64 of its in it ial va lue in th is first-order reaction?
Rate information was obtained for the following reaction at 25°C and 33°C; Cr(H2O)6 3+ + SCN¯ ---> Cr(H2O)5NCS2+ + H2O(l) Initial Rate [Cr(H2O)6 3+] [SCN-] @ 25°C 2.0x10-11 1.0x10-4 0.10 2.0x10-10 1.0x10-3 0.10 9.0x10-10 2.0x10-3 0.15 2.4x10-9 3.0x10-3 0.20 @ 33°C 1.4x10-10 1.0x10-4 0.20 Can a 4th order reaction occur?
Rate information was obtained for the following reaction at 25°C and 33°C; Cr(H2O)6 3+ + SCN¯ ---> Cr(H2O)5NCS2+ + H2O(l) Initial Rate [Cr(H2O)6 3+] [SCN-] @ 25°C 2.0x10-11 1.0x10-4 0.10 2.0x10-10 1.0x10-3 0.10 9.0x10-10 2.0x10-3 0.15 2.4x10-9 3.0x10-3 0.20 @ 33°C 1.4x10-10 1.0x10-4 0.20 a) Write a rate law consistent with the experimental data. b) What is the value of the rate constant at 25°C? c) What is the value of the rate constant at 33°C? d) What is the activation energy for this reaction? e) Can a 4th order reaction occur?
The acid-catalyzed hydrolysis of sucrose occurs by the fol-lowing overall reaction whose kinetic data are given below:C₁₂H₂₂O₁₁(s) H₂O(l) →C₆H₁₂O₆(aq) C₆H₁₂O₆(aq) (a) Determine the rate constant and the half-life of the reaction.(b) How long does it take to hydrolyze 75% of the sucrose?(c) Other studies have shown that this reaction is actually sec-ond order overall but appears to follow first-order kinetics.(Such a reaction is called a pseudo–first-order reaction.) Sug-gest a reason for this apparent first-order behavior.
The value of ΔS° for the catalytic hydrogenation of acetylene to ethane, C2H2 (g) + 2H2 (g) → C2H6 (g) is __________ J/K∙ mol. A) -76.0 B) +440.9 C) -232.5 D) +232.5 E) +28.7
A+B➡️P t=0 :C(A)=C(B) t=500sec 20% of react t=? Sec 60% of compl

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Vilsmeier Rea میکانزم ا CHO استخدم POCI DMF VILSMEIER CHO H ے