Question

What is the difference between zero-order and first-order kinetics?

Answer 1

Order of a reaction:

1. A chemical reaction's order can be defined as the sum of powers of the concentration of the reactants in the rate law expression.
2. For example, the rate of a reaction is $\mathrm{Rate}=\mathrm{k}{\left[\mathrm{A}\right]}^{\mathrm{x}}{\left[\mathrm{B}\right]}^{\mathrm{y}}$, where x and y are the order of the reactants A and B. The overall order of this equation is $\mathrm{x}+\mathrm{y}$.

Zero-order kinetics:

1. The rate of reaction is proportional to the zero power of the reactant concentration.
2. An order of a reaction is determined for a reaction by analyzing the graph between the concentration of reactant and time.
3. The rate expression of the zero-order kinetics is: $\mathrm{Rate}=\mathrm{k}{\left[\mathrm{R}\right]}^0$, where k is a rate constant and R is a reactant concentration.
4. The slope and intercept of this reaction are $-\mathrm{k}$ and initial concentration of reactant ${\left[\mathrm{R}\right]}_0$.

First-order kinetics:

1. The order of a reaction is proportional to the first power of the reactant concentration.
2. An order of a reaction is calculated by a creation by using a graph between logarithmic reactant concentration and time.
3. The rate expression of first-order kinetics is: $\mathrm{Rate}=\mathrm{k}\left[\mathrm{R}\right]$.
4. The slope and intercept of this reaction are $-\mathrm{k}$ and $\ln {\left[\mathrm{R}\right]}_0$.