Some Exam Questions on Kinetics (EYRING Theory, BODENSTEIN's Steady-State Approximation)
This is a modal window.
The media could not be loaded, either because the server or network failed or because the format is not supported.
Formal Metadata
| Title |
| |
| Title of Series | ||
| Number of Parts | 34 | |
| Author | 0000-0002-4319-5413 (ORCID) | |
| Contributors | ||
| License | CC Attribution - NonCommercial 3.0 Germany: You are free to use, adapt and copy, distribute and transmit the work or content in adapted or unchanged form for any legal and non-commercial purpose as long as the work is attributed to the author in the manner specified by the author or licensor. | |
| Identifiers | 10.5446/34677 (DOI) | |
| Publisher | 0000-0002-4319-5413 (ORCID) | |
| Release Date | ||
| Language |
Physical Chemistry11 / 34
00:00
Transition metalChemical reactionSteadystate <Physiologie>Mortality rateHuman body temperatureSolventChemical reactionIonenstärkeReaction rate constantExothermieSolventHuman body temperatureOctane ratingSunscreenConcentrateIronMultiprotein complexEnzymkinetikNanoparticleLecture/Conference
Transcript: English(auto-generated)
00:00
This exam question is about the kinetics of complex reactions and the iron theory. The concentration of an unstable intermediate is very low and approximately constant. This statement is correct.
00:21
It's equivalent to Burdenstein's steady-state principle. A catalyst accelerates the rate of the reverse reaction by the same factor as the rate of the forward reaction. This is a correct statement, too. Otherwise, the catalyst would change equilibrium.
00:46
Temperature increase accelerates the rate of the forward reaction of an exothermic equilibrium more than the rate of the reverse reaction. This is correct. It is the reason for the equilibrium of an exothermic reaction to be shifted to the left-hand side at higher temperature.
01:09
At equilibrium, the rate constants of the forward reaction and the reverse reactions are equal. This statement is not correct. At equilibrium, also the rates of the forward and the reverse reactions are the same.
01:26
At equilibrium, the rate constants are usually different. Reactions between like-charged ions are faster in non-polar solvents than in polar solvents. If you look at the Brønsted-Christiansen-Sketcher equation we see that in reactions with like-charged particles
01:48
the rate constant increases when we either work in polar solvents or at higher ionic strength. Reactions between like-charged ions are faster at higher ionic strength than at low ionic strength.
02:08
This is correct, too. Thanks for watching.