Sample Jones Test 1 HO A 2345 2 4 CH3 Blue-green precipitates No reaction No reaction No reaction Blue-green precipitates H3C CH3 B LOH Lucas test No reaction Cloudiness No reaction No reaction Cloudiness OH с OH lodoform test No reaction No reaction No reaction No reaction Yellow precipitates H₂C OH D CH 3 FeCl3 test No reaction No reaction No reaction Violet color No reaction E

Sample Jones Test 1 HO A 2345 2 4 CH3 Blue-green precipitates No reaction No reaction No reaction Blue-green precipitates H3C CH3 B LOH Lucas test No reaction Cloudiness No reaction No reaction Cloudiness OH с OH lodoform test No reaction No reaction No reaction No reaction Yellow precipitates H₂C OH D CH 3 FeCl3 test No reaction No reaction No reaction Violet color No reaction E

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 3QAP: How do chemists envision reactions taking place in terms of the collision model for reactions? Give...

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Similar questions

In general, can we predict the effect of doubling the concentration of A on the rate of the overall reaction A+BC? Can we predict the effect if the reaction is known to be an elementary reaction?
Define these terms: (a) unimolecular reaction (b) bimolecular reaction (c) elementary reaction (d) overall reaction
How do chemists envision reactions taking place in terms of the collision model for reactions? Give an example of a simple reaction and how you might envision the reaction’s taking place by means of a collision between the molecules.
Why awe elementary reactions involving three or more reactants very uncommon?
In terms of collision theory, to which of the following is the rate of a chemical reaction proportional? (a) the change in free energy per second (b) the change in temperature per second (c) the number of collisions per second (d) the number of product molecules
Consider the hypothetical reaction A+B+2C2D+3E In a study of this reaction three experiments were run at the same temperature. The rate is defined as [B]/t. Experiment 1: [A]0 = 2.0 M [B]0 = 1.0 103 M [C]0 = 1.0 M [B] (mol/L) Time(s) 2.7 104 1.0 105 1.6 104 2.0 105 1.1 104 3.0 105 8.5 105 4.0 105 6.9 105 5.0 105 5.8 105 6.0 105 Experiment 2: [A]0 = 1.0 102M [B]0 = 3.0 M [C]0 = 1.0 M [A] (mol/L) Time(s) 8.9 103 1.0 7.1 103 3.0 5.5 103 5.0 3.8 103 8.0 2.9 103 10.0 2.0 103 13.0 Experiment 3: [A]0 = 10.0 M [B]0 = 5.0 M [C]0 = 5.0 101M [C] (mol/L) Time(s) 0.43 1.0 102 0.36 2.0 102 0.29 3.0 102 0.22 4.0 102 0.15 5.0 102 0.08 6.0 102 Write the rate law for this reaction, and calculate the value of the rate constant.