integrated rate equation for first order
Answers
You must already know that calculating the rate of a reaction is extremely important to understand the reaction. But it also necessary to infer the rate law of a reaction to find out the order of the reaction. But what is the order of a reaction you ask? Let’s find out below and also learn about the different types of reactions.
We know that the rate law is the expression in which reaction rate is given in terms of molar concentration of reactants with each term raised to some power, which may or may not be equal to the stoichiometric coefficient of the reacting species in a balanced chemical equation.
Consider a general reaction, aA + bB → cC + dD where a, b, c, d are the stoichiometric coefficients of the reactants and the products. Therefore, the rate law for the above reaction is,
Rate ∝ [A]x [B]y
where x and y may or may not be equal to the stoichiometric coefficients of the reactants. Therefore, the rate of the reaction is equal to k [A]x [B]y, where k is the rate constant.
∴ -d[R]/dt = k [A]x [B]y
The order of a reaction is the sum of the powers of the concentrations of the reactants in the rate law expression. In the above general reaction, x and y are the powers. The sum of them will give the order of the reaction. Order of a reaction can be 0, 1, 2, 3 and even a fraction. A zero-order reaction means that the rate of the reaction is independent of the concentration of reactants.
You must already know that calculating the rate of a reaction is extremely important to understand the reaction. But it also necessary to infer the rate law of a reaction to find out the order of the reaction. But what is the order of a reaction you ask? Let’s find out below and also learn about the different types of reactions.
We know that the rate law is the expression in which reaction rate is given in terms of molar concentration of reactants with each term raised to some power, which may or may not be equal to the stoichiometric coefficient of the reacting species in a balanced chemical equation.
Consider a general reaction, aA + bB → cC + dD where a, b, c, d are the stoichiometric coefficients of the reactants and the products. Therefore, the rate law for the above reaction is,
Rate ∝ [A]x [B]y
where x and y may or may not be equal to the stoichiometric coefficients of the reactants. Therefore, the rate of the reaction is equal to k [A]x [B]y, where k is the rate constant.
∴ -d[R]/dt = k [A]x [B]y
The order of a reaction is the sum of the powers of the concentrations of the reactants in the rate law expression. In the above general reaction, x and y are the powers. The sum of them will give the order of the reaction. Order of a reaction can be 0, 1, 2, 3 and even a fraction. A zero-order reaction means that the rate of the reaction is independent of the concentration of reactants.