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- Define chemical kinetic and reason that why it is studied
- Average and instantaneous rate of reaction along with the graphical representation
- Relation between chemical kinetics and thermodynamics
- Expression of average rate of reaction for a reaction
- Significance of minus sign with the concentration of reactant
- Unit of rate of reaction
- Factor influencing the rate of reaction
- Define rate law and rate constant along the expression
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- Order of reaction and its application
- Difference between elementary and complex reaction
- Unit of rate constant for different order of reactions
- Difference between order and molecularity of reaction
- Why the slowest step is consider as rate determining step?
- For a reaction, A + B --------> Product; the rate law is given by, r = k [A]1/2 [B]2.What is the order of the reaction?
- Determination of zero order reaction and Variation in the concentration vs time plot for a zero order reaction to fined the slop of the zero order reaction
- A plot between ln[R] and t for a first order reaction to fined the slope
- Fined the slope of first order reaction from plot of log [R]0 /[R] vs time
- The initial concentration of N2O5 in the following first order reaction N2O5(g) ----------> 2 NO2(g) + 1/2O2 (g) was 1.24 × 10–2 mol L–1 at 318 K. The concentration of N2O5 after 60 minutes was 0.20 × 10–2 mol L–1.Calculate the rate constant of the reaction at 318 K.
- Relation between rate constant and half life for zero and first order reaction
- What do you mean by pseudo first order reaction? Define by taking one example
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- How rate of reaction depends on temperature? Explain
- Relation between rate of reaction and Arrhenius factor or the frequency factor or pre-exponential factor.
- Define most probable kinetic energy and formation of activated complex
- Explain the effect of catalyst on rate constant by plotting a graph between potential energy and reaction coordinate
- A substance reacts according to the first order kinetics and rate constant for the reaction is 1x 10-2 Sec-1. If initial concentration is 1M. Find out the rate of reaction after 1 minute.
- The rate of a reaction becomes four times when the temperature changes from 293 K to 313 K. Calculate the energy of activation (Ea) of the reaction assuming that it does not change with temperature. [R = 8.314 J/K mol, log 4 = 0.6021
- Define collision frequency
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