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Mindmap: Chemical Kinetics | Chemistry Class 12 - NEET PDF Download
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FAQs on Mindmap: Chemical Kinetics - Chemistry Class 12 - 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 them. It involves understanding how reactants transform into products over time and the factors that affect the speed of these reactions.
| 2. What are the factors that affect the rate of a chemical reaction? | |
Ans. Several factors can influence the rate of a chemical reaction, including the concentration of reactants, temperature, presence of a catalyst, surface area of the reactants, and the nature of the reactants. These factors can either increase or decrease the rate of the 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. The initial rate of the reaction is often determined by measuring the change in concentration of a reactant or product at the beginning of the reaction. The rate can also be determined by monitoring other properties such as color change or gas evolution.
| 4. What is the rate law of a chemical reaction? | |
Ans. The rate law of a chemical reaction expresses the relationship between the rate of the reaction and the concentrations of the reactants. It is determined experimentally and is often expressed in the form of a mathematical equation, where the rate is proportional to the concentrations of the reactants raised to certain powers, known as the rate constant.
| 5. What is the effect of temperature on the rate of a chemical reaction? | |
Ans. Temperature has a significant effect on the rate of a chemical reaction. Increasing the temperature generally increases the rate of a reaction, as it provides more kinetic energy to the reactant molecules, leading to more frequent and energetic collisions. This increase in collision frequency and energy allows for more successful collisions, resulting in a faster reaction rate.
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