Chm 116 Lab
INTRODUCTION
Chemical kinetics, which can also be explained as reaction kinetics, studies the rates of chemical processes and reactions. A lot of this has to do with the speed at which a chemical reaction occurs for instance the rate at which reactants and products appear and disappear. In this case chemical kinetics goes further in depth to understand what conditions affect the rate of a given reaction. This is important because it allows scientists to determine what type of reaction can occur, and how they can alter the outcome under varying conditions. Gasoline and diesel for example have two very different reaction rates when exposed to a spike in temperature. If you were to light gas on fire it would instantaneously explode igniting fumes in the air as well, however diesel has a much higher ignition temperature allowing it to slowly burn if lit. These two types of fuel are an example of the differences in reaction rate. To determine the rate at which these reactions occur we use the rate law: r=kAxBy. In this equation we are looking to solve for the rate of the reaction “r”, the k value which represents our rate constant is simply the value which quantifies the speed. As for the [A] and [B] values they are the concentration of the species A and B which respectively are raised to the “x” and “y” power. The “x” and “y” values are the respective stoichiometric coefficients that must be determined experimentally. The primary goal essentially for this experiment is to determine the k value or rate constant along with the x and y stoichiometric coefficients given the concentrations of Crystal Violet and Hydroxide. This can be obtained using a spectrophotometer to determine rate of absorbance then graph the rate find a line of best fit, determine our rate constant, then finally solve for our x and y in the rate law equation. Beer’s law also known as Beer-Lambert law relates the absorption of light to the properties of the material through which the
Chemical kinetics, which can also be explained as reaction kinetics, studies the rates of chemical processes and reactions. A lot of this has to do with the speed at which a chemical reaction occurs for instance the rate at which reactants and products appear and disappear. In this case chemical kinetics goes further in depth to understand what conditions affect the rate of a given reaction. This is important because it allows scientists to determine what type of reaction can occur, and how they can alter the outcome under varying conditions. Gasoline and diesel for example have two very different reaction rates when exposed to a spike in temperature. If you were to light gas on fire it would instantaneously explode igniting fumes in the air as well, however diesel has a much higher ignition temperature allowing it to slowly burn if lit. These two types of fuel are an example of the differences in reaction rate. To determine the rate at which these reactions occur we use the rate law: r=kAxBy. In this equation we are looking to solve for the rate of the reaction “r”, the k value which represents our rate constant is simply the value which quantifies the speed. As for the [A] and [B] values they are the concentration of the species A and B which respectively are raised to the “x” and “y” power. The “x” and “y” values are the respective stoichiometric coefficients that must be determined experimentally. The primary goal essentially for this experiment is to determine the k value or rate constant along with the x and y stoichiometric coefficients given the concentrations of Crystal Violet and Hydroxide. This can be obtained using a spectrophotometer to determine rate of absorbance then graph the rate find a line of best fit, determine our rate constant, then finally solve for our x and y in the rate law equation. Beer’s law also known as Beer-Lambert law relates the absorption of light to the properties of the material through which the