What are chemical kinetics?- Chemarticle.com| class note pdf

Introduction

Hello everyone, today we will discuss chemical kinetics reactions. We are providing the chemical kinetics formula, Chemical kinetics note PDF, Chemical kinetics MCQ For class 12th. What is the chemical Kinetic definition we will discuss briefly?

Also, we will provide the chemical kinetics NCERT PDF. Chemical kinetics question with solution pdf Provide in this Article this chemarticle.com. This chemical kinetics Portion of physical chemistry is very important for CSIR NET,  GATE, IIT JAM, TIFR, MSc entrance, BARC Examination. We are providing the PDF note for helpful content of these Chem Articles. 

Chemical kinetics

Hello everyone, today we will Discuss chemical kinetics. Chemical kinetics is a very very important topic in physical chemistry. It is the concept of measurement of the rate of a reaction given under conditions of temperature, pressure, and concentration of reactant. The study of chemical kinetics is very very useful for reaction steps for understanding mechanisms. We briefly discuss chemical kinetics and their separate order for reaction. Chemical studies is a modern theory. We have to use the Chemical synthesis product to get the maximum yield. They have various uses for industrial product formation. They have required for or better of the reaction product. 

Thermodynamically which can predict at room temperature hydrogen and oxygen react with and formation of water. But how many times are required for this reaction information of water molecules we cannot predict.  In cases, chemical kinetics plays a very very important role in this situation or in modern chemistry. In chemical kinetics how many times are required for completing a reaction to form a product we can easily predict. 

Study of chemical Kinetic reaction

All experimental techniques have been developed to monitor the concentration of reaction and the reactant product there several times are required. 

For the reaction One or more product formation in cases into N2O5 is gases reactant To produce Two gaseous products NO2 gas and O2 gas.

Rate of reaction

Consider a simple reaction A to P formation where a is reactant and P is the product. The rate of the reaction is at a certain time of the reactant concentration. We get the rate expression-

r= -d[A]/dt

Where [A] is the concentration of A at time t. The concentration of reactant A will decrease when Increase the reaction time t. 

The rate law and rate constant

The reaction A to P product formation the rate expression  get 

  r= k[A] Where K is the rate constant or velocity constant. When unity concentration of the reactant the rate is equal to the rate constant of this reaction. That means the concentration of a is equal to one then the rate constant is equal to the rate of this reaction. [A]=1, Scenes we can get  r=k. K is the rate constant of this reaction.

Order of a reaction

In the study of chemical kinetics, The classification of the reaction will be indicated by the order of the reaction. The order of the reaction is a defined sum of power in reactant concentrations called the order of this reaction. That means the power of concentration of A is equal to 2 which means the order of this reaction is the second-order reaction. 

According to the Rate Law equation, we can classify the order of the reaction firstly the power of concentration equals 0,1,2,3,4…… When the power of concentration equals zero that means the rate of the reaction equals rate constant that does not depend on reactant concentration. 

We are studying chemical kinetics to Zero order reaction, first-order reaction, second-order reaction. 

Define rate expression for the zero-order reaction

For example, zero-order reaction A to P product formation. 

A➡P

 r= -d[A]/dt =k0 where k0 is Rate constant of zero-order reaction.

If at t=o, the Initial concentration of A is [A]0  and concentration at time t is equal to t  is [A]. then we get...

The chemical kinetics rate equation for the zero-order reaction: grave plot rate vs time, the concentration of reactant vs time. where slope=k, which is the rate constant of the reaction.

So, that we can calculated this value get , k0 = 1/t([A]0 - [A]) 

This is the Rate equation of the zero-order reaction. This is the chemical kinetics Formula of zero-order reaction. 

First-order reaction

Consider the first-order reaction rate expression for A to P formation.

 

Chemical kinetics: first-order reaction 

In a first-order reaction, the concentration of the reactant is decreased when time is increased. Their product will increase exponentially Corresponding to time. An example of a first-order reaction is N2O gas decomposes into N2 gas and O2 gas form.

Conclusion

We are hopeful that understand this speech Article on chemical kinetics. We are discussing the physical person of the chemical kinetics definition in this article very briefly. That is the basic concept of chemical kinetics. Chemical kinetics class 12 to graduation all are the same physical portion. This is the chemical kinetics-1 introduction class of chemical kinetics. Thank you for reading.

Frequently asked question

Q1. What is the chemical kinetics definition?

Ans: A product formation how many times are required for a reactant to product transformation that is calculated by chemical kinetics. Chemical kinetics is the reaction of the reactant transformation rate of the reactant to the product. It is considered the measurement of the rate of the reaction under the condition of temperature pressure and concentration of the reactant or product. That is the chemical kinetics definition.

Q2. What is the chemical kinetics application?

Ans:  mainly thermodynamics Predict the product formation produced or not.  but how many times are required for a reaction is not predicted in these thermodynamic systems.  In case chemical kinetics are done to predict the product how many times are required. So their application will play a very important role in the Chemical synthesis of the reaction.

Q3. What do you mean chemical kinetics class 12th?

Ans: The chemical kinetics of the basic concept for zero order, first order, and second-order reaction provides the chemical kinetics class 12th. Also, we provide the half-life time of a reaction. Or how many times are required for a Given concentration reactant to form a product. Concept of what is the chemical Kinetic Rate Law equation. Concept of Rate expression of a reaction. It may be first-order, zero-order, or second-order reactions. 

Q4. What are the chemical kinetics topics?

Ans: First of all we understand chemical kinetics reactions. Then Rate of reaction, Rate Law and Rate constant,  order of a reaction, Unit of a rate constant, Zero-order, first-order, second-order reaction, etc all understood in the chemical kinetics topic. Then we will understand the half-life time of a reaction. How to change the half-life in changing the order of the reaction. Arrhenius equation solving for a certain reaction given by their activation energy.

Q5. Why does the first-order reaction not complete?

Ans: We can see that in the first-order reaction half-life does not depend on the concentration of the reactant.  which is a Defined only one rate constant of the reaction. The first-order reaction does not depend on the concentration of the reactant. That means we can see that the first-order reaction completes in infinite time.

Why does the first-order reaction not complete? Chemical kinetics rate equation.

Q6. What is the half-life time of a first-order reaction?

Ans: The time required for The first-order reaction is 50% Complete, Which Time is called the half-life time of this reaction. At times t is equal to zero When the concentration of  Reactance is [N]0, This is the initial concentration of reactant. For the half lifetime or 50% complete the reaction time is t =t1/2 then the concentration of reactant is [N]=[N]0/2. Now we are put into the first-order reaction rate equation k= 1/t ln([N]0/[N]). We get k= 1/t1/2 ln(([N]0/([N]0/2)). Solve the equation and get the t half value equals 0.693/K. Since Half lifetime of the reaction t1/2=0.693/k.

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