Describe the differences between zero, first, and second order reactions.

Zero, first, and second order reactions differ in their rate of reaction with respect to the concentration of reactants.

Zero order reactions have a constant rate of reaction, independent of the concentration of reactants. This means that the rate of reaction remains the same even if the concentration of reactants changes. Examples of zero order reactions include the breakdown of alcohol by the liver and the decomposition of hydrogen peroxide by catalase.

First order reactions have a rate of reaction that is directly proportional to the concentration of one reactant. This means that the rate of reaction increases as the concentration of the reactant increases. Examples of first order reactions include radioactive decay and the hydrolysis of esters.

Second order reactions have a rate of reaction that is directly proportional to the concentration of two reactants or the square of the concentration of one reactant. This means that the rate of reaction increases as the concentration of the reactants increases or as the square of the concentration of one reactant increases. Examples of second order reactions include the reaction between hydrogen ions and hydroxide ions to form water and the reaction between iodine and propanone.

Understanding the order of a reaction is important in determining the rate of reaction and the concentration of reactants needed to achieve a desired rate. It also helps in predicting the effect of changing the concentration of reactants on the rate of reaction.