Reaction Kinetics Essay -- essays research papers

Reaction Kinetics Rate of ReactionOf Tertiary-Butyl banalityPurpose The purpose of this prove is to let the order of t-BB graphically, to find the k ( order constant) at 0&730 C and at room temperature, also to find the Ea (activation postcode).Principles Several different chemical kinetic principles were used in this experiment. The reception rates of this chemical equation were determined experimentally. This then allowed the reaction mechanisms (i.e. orders of from each one component, rate constant, etc.). These mechanisms were ultimately determined to be compiled to form a rate law. Rate = kAmBnIntegrated rate laws are used to determine concentrations of reactants at certain times. However, these integrated equations can only be used subsequently the experimental data is collected. Temperature has an effect on the rates of reactions. Swedish chemist, Svante Arrhenius, ascertained that the rate constant of a reaction increased logarithmically in proportion to the reciproca l of the absolute temperature. This is expressed mathematically ask = Ae-&916E/RTMethod 100 mL of water/ Isopropyl Alcohol were added to a 250 mL Earlenmeyer flaskful along with 15 drops of phenolphthalein. A buret was washed with soapy water and rinsed with 0.2 M NaOH. The buret was then filled to 0.00 mL. 2.00 mL of NaOH were added to the flask and it was placed into an ice-water bath.t-BB was injected into the flask by the lab assistant with this involve time being noted. The exact time was memorialise once once again when the solution became colorless.About two mL of NaOH were added to the solution and the time recorded when this became colorless. This was done until seven time readings were recorded. After the 7th addition of NaOH, the flask was withdraw from the ice bath and placed in a earnest water bath for approximately ten minutes. The flask was then removed from the bath and cooled to room temperature. The solution was then titrated to a slight ping color. The volu me reading of the burette was equal to the total base added during the experiment. This experiment was repeated in duplicate at room temperature.CH3 CH3CH3 - C - Br + H2O &61664 CH3 - C - OHCH3 CH3T... ...found to be the 1/H graphs. This means that the reaction was a simple second order reaction.Rate Constant Calculations A. (11.90-5.29)/(2687-160) = 2.62x10-3 B. (10.00-4.65)/(191-25) = 3.22x10-2 activation Energy Calculation ln(k2 k1) = -(&916E/8.314) (1/T2 1/T1) Ea = -8.312 (lnK2 lnK1) / (1/T2 1/T1) = -8.314 (ln 3.22x10-2 ln 2.62x10-3) / (1/298.15 1273.15) = 67.3 KJ/mol resultant This reaction was found to be simple second order. The rate constants were 2.62 x 10-3 at 0 degrees C, and 3.22 x 10-2 at room temperature. The activation energy was calculated to be 67.3 KJ/mol. There were no unusual problems encountered during this experiment. Error in data may be due to lack of ability to record times accurately.