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Fun Video: Overview of Chemical Kinetics Video Lecture - NEET
FAQs on Fun Video: Overview of Chemical Kinetics Video Lecture - NEET
| 1. What is chemical kinetics? |  |
Ans. Chemical kinetics is the branch of chemistry that deals with the study of the rates of chemical reactions and the factors that influence these rates. It involves the analysis of how fast a reaction occurs, the mechanisms that govern the reaction, and the factors that can speed up or slow down the reaction.
| 2. What are the factors that affect the rate of a chemical reaction? | |
Ans. Several factors can influence the rate of a chemical reaction. These factors include temperature, concentration of reactants, presence of a catalyst, surface area of reactants, and pressure (in the case of gases). Increasing the temperature, concentration, or surface area, and adding a catalyst can all generally increase the rate of a reaction.
| 3. How is the rate of a chemical reaction determined experimentally? | |
Ans. The rate of a chemical reaction can be determined experimentally by measuring the change in concentration of a reactant or product over time. This can be done using various techniques such as spectrophotometry, titration, or monitoring the release of gases. By plotting the concentration versus time, the rate can be determined from the slope of the resulting curve.
| 4. What is the order of a chemical reaction? | |
Ans. The order of a chemical reaction refers to the dependence of the reaction rate on the concentration of the reactants. It can be determined experimentally by conducting multiple trials with different initial concentrations of reactants and observing how the rate changes. The order can be zero, first, second, or even fractional, depending on the rate equation derived from the experimental data.
| 5. How does a catalyst affect the rate of a chemical reaction? | |
Ans. A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It achieves this by providing an alternative reaction pathway with a lower activation energy. This lowers the energy barrier for the reaction, allowing more reactant molecules to overcome it and thus increasing the rate of the reaction.
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