Determination of the Rate Constant
Determination of the Rate Constant for a Chemical Reaction
Department of Chemistry
Abstract
This experiment was performed to determine the rate constant k, for hydrolysis of tertiary butyl chloride to tertiary butanol. The solvent system for this reaction is 45% isopropyl alcohol and 55% water. The rate of hydrolysis of t-butyl chloride is measured by the decrease in the concentration of this reagent with time. The rate of decomposition of t-butyl chloride must be equal to the rate of formation of hydrochloric acid. The rate of hydrochloric acid formation was measured by titrating the acid produced with a base, NaOH.
Introduction
The field of chemical kinetics studies the speed of chemical reactions and the reasons that affect the speed of a reaction. The speed of a chemical reaction is usually called the reaction rate. The reaction rate is defined as the change in concentration of a reactant's or a product's concentration per unit time. It is defined so that you will gain the same rate no matter which species in a chemical reaction is chosen. For this experiment, the rate of hydrochloric acid formation was measured by titrating the acid produced with a base. The order of reaction, as carried out by this method is first order. This reaction is first order because of the large excess of water present in the reaction mixture. The concentration of water does not change to any considerable extent during the reaction and does not appear in the rate law. This experiment was an intermediate event and such a reaction is most often called hydrolysis and is represented by the equation:
C4H9Cl + H2O C4H10O + HCl.
Experimental
A burette was rinsed with 0.25M sodium hydroxide. The burette was drained and refilled with the sodium hydroxide solution. 100mL of isopropyl alcohol/water solvent was placed in a 100 mL volumetric flask. This solution was put into a 250 mL flask in a constant temperature water bath and the temperature of the bath and the
Department of Chemistry
Abstract
This experiment was performed to determine the rate constant k, for hydrolysis of tertiary butyl chloride to tertiary butanol. The solvent system for this reaction is 45% isopropyl alcohol and 55% water. The rate of hydrolysis of t-butyl chloride is measured by the decrease in the concentration of this reagent with time. The rate of decomposition of t-butyl chloride must be equal to the rate of formation of hydrochloric acid. The rate of hydrochloric acid formation was measured by titrating the acid produced with a base, NaOH.
Introduction
The field of chemical kinetics studies the speed of chemical reactions and the reasons that affect the speed of a reaction. The speed of a chemical reaction is usually called the reaction rate. The reaction rate is defined as the change in concentration of a reactant's or a product's concentration per unit time. It is defined so that you will gain the same rate no matter which species in a chemical reaction is chosen. For this experiment, the rate of hydrochloric acid formation was measured by titrating the acid produced with a base. The order of reaction, as carried out by this method is first order. This reaction is first order because of the large excess of water present in the reaction mixture. The concentration of water does not change to any considerable extent during the reaction and does not appear in the rate law. This experiment was an intermediate event and such a reaction is most often called hydrolysis and is represented by the equation:
C4H9Cl + H2O C4H10O + HCl.
Experimental
A burette was rinsed with 0.25M sodium hydroxide. The burette was drained and refilled with the sodium hydroxide solution. 100mL of isopropyl alcohol/water solvent was placed in a 100 mL volumetric flask. This solution was put into a 250 mL flask in a constant temperature water bath and the temperature of the bath and the
References: Experiment 3 https://blackboard.cwidaho.cc/webapps/portal/frameset.jsp?tab_tab_group_id=_2_1&url=%2Fwebapps%2Fblackboard%2Fexecute%2Flauncher%3Ftype%3DCourse%26id%3D_1880_1%26url%3D N.p., n. d. Web. 28 Sep. 2013. .