Kinetics lab report

Document Type:Lab Report

Subject Area:Chemistry

Document 1

You are unable to deduce anything about the order of a reaction just by looking at the equation for the reaction. The rate of reaction would be written as rate=k[A]^2 where the 2 is the order of reaction. In this case, the reaction is order 2 for A, its second order reaction for any element A. the calculations of the order of reaction and rate constants from the given data or experiments. The rate of reaction and the value of the rate constant at 28 degrees or group 1a to 4b; CH3COCH3 + Br3-----H+-----> CH3COCH2Br + HBr After 3 or 4 trials the order of the reaction will be [CH3COCH3] ^B. 1exp-0. 6exp-0. 05] ^C which leads us to evaluation of C directly.

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C= log (4. 07)/log 4 = 1, thus 1 is the kinetic order of hydrogen ions. 6 M The group 1a to 4a help us calculate the value of the order of reaction from the three trials conducted. The blue dye is added to bromine water to end up with the last orders of reaction found above. Kinetics Energy of Activation The activation energy of a chemical reaction is related to its rate. The higher the activation energy, the slower the chemical reaction will be. The molecules can only complete the reaction when they have reached the top of the activation energy barrier. 075L= 0. 0573M For run 1 at T=0=273K t= 813. 6 seconds R= = 1/2= = 0. 0021M/s (ii) Determination of k [I-] = 0. 0300L*0. 9kJ/mol In conclusion, the rate of the chemical reaction is highly dependent on the temperature at which the experiment is done.

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