Basic-Gyan

Both methods are used to calculate the reaction order in a reaction or to analysis the kineti c data. The " Differential Method " directly deals with the rate law written for a given reaction. While the " Integral Method " is a hit and trial method in which we substitute the values of the concentrations and time and then we check whether the rate equations are satisfied with these values or not.  The integrated rate law equation expresses the concentration of the reactant as a function of time. And the order and rate constant of the reaction can be found from the integrated rate law equation. This is done by substituting the concentration versus time data in various integrated rate law equations, checking whether all calculated "k" values ​​are the same. Either  the " Differential And Integral Rate Law Equation " is used to determine the reaction order.  Let Us Define Both Methods One By One - Differential Rate Law " The differential rate l...

Fig:- Reaction Energy Diagram   In the above figure, this enthalpy change in energy between reactants and products is called " Heat Of Reaction ".  The value of the heat of reaction determines whether the reaction is exothermic or endothermic. Besides activation and threshold energy, another form of energy exists here and that is " Heat Of Reaction ". It is also known as " Enthalpy Change ". It is defined as the net amount of energy that should be added or released during a chemical reaction. Figure-1 Figure-2 In the above figure, energy of the reactants and the energy of the products are not the same, but there are some differences between them. And this difference represents the heat of the reaction.  Hence, " Heat  of a reaction is defined as the difference between the average energy of the reactants and the average energy of the products ".  This difference can be positive or negative. And depending on these positive and negative values of th...

We all must have heard about " Threshold Energy " and " Activation Energy ". So let us now see the difference between threshold energy and activation energy.  From ' Collision Theory ', we know that a reaction occurs when the reactant molecules collide with each other and these collisions must be an effective collision so that the reaction can occur. The collision are an effective collision if the reactant molecules must have energy more than threshold energy. Reactant molecules have low energy at room temperature due to which their collisions are not effective and reactants do not convert into products. In this situation, we give energy (or activation energy) to reactant molecules in the form of heat, light etc. So that they absorbs this energy and their energy becomes equal to or greater than threshold energy. As a result, the reactant is easily converted into products by effective collisions.   Thus, " Threshold energy is the summation of the avera...

When a reaction goes to completion then the reactant present in the reaction is converted into product by passing through the activated state (or the highest energy level in the reaction energy diagram). And to overcome this activated state (which is the highest energy point in the reaction energy diagram), reactant molecules must have enough energy so that they can be easily converted into products and that much amount of energy required by the reactant molecules to overcome this activated state is called as " Activation Energy ". Thus, activation energy is the minimum amount of energy needed to start a chemical reaction. Thus, we can define the activation energy as; " Activation Energy is the least possible amount of energy required by the reactant molecules to start a chemical reaction ". And activation energy is usually expressed in calories or joules per mole. For Example Burning of woods using lighter. Here, the energy given off by the lighter is nothing but t...

" Chemical Kinetics " also known as " Reaction Kinetics " which helps us to understand the rate of chemical reactions (or reaction rate) and tells us how these rates influenced by certain conditions.  For Examples :  Some reactions are happened at a faster rate (like in few second) while others are happened at a very slow rate (like in many days).  Rusting of iron - At a slow rate Wood combustion - At a fast rate  Nuclear explosion- At a fast rate Hence, the rate of reaction (at which a reaction goes to completion) can change according to the condition through which the reaction occurs.   In this article, we will learn about the factors which affects the rate of reaction . Rate Law Let us define a " Rate Law " which tell us about the rate of reaction and also tell us that these rates are affected by which parameters, " A rate law or a rate equation is a relationship between the reaction rate and the concentration of its reactants ". Thus, a reac...

I will like to tell you first the definition of the two terms ' specific heat ' and ' latent heat '.          " Specific heat is amount of heat required to raise the temperature of 1kg of substance by one degree Celsius ". While " Latent heat is amount of heat required to change the state of substance without increase in temperature ".           One more thing is that steam is a gaseous form of water. Thus, when water gets converted into steam, it absorbs latent heat. It's heat content (or simply say enthalpy) increases not the temperature. While water from 25 to 100°C (degree Celsius) absorbs specific heat, it doesn't have latent heat.           Thus; steam has more heat content than water at 100 degree Celsius.     Water- 25to100°C - Contain specific heat only  Steam- 25to100°C - Contain (specific+Latent) heat Hope you have found this article helpful!! Do you have suggestions? Please write in com...

We know that when a reaction is completed, all the reactants are completely converted into products. But the reactants do not directly convert into products. Rather, the reactants first convert to the transition state, and then from the transition state to the intermediate, then from the intermediate to the second transition state, and finally from the second transition state to the product.   Hence " Intermediates are defined as a molecular entity which is formed inbetween reactants and products (It is neither be a reactant nor a product) or inbetween two transition states ". Fig:- Reaction Energy Diagram   In a reaction mechanism (series of elementary reactions through which the overall reaction takes place), intermediate molecule is formed in one elementary step while consumed in another elementary step. Therefore, these intermediates are not present in the overall balanced equation. But still a part of every reaction. Intermediates tend to be extremely reactive due to the...