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    Objective: Apparatus Required:: Experiment#3

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    Fahad kamran
    This experiment aims to determine the kinetics law parameters (reaction order n and rate constant k) of a chemical reaction between sodium hydroxide and ethyl acetate using the integral method of analysis. Conductivity readings of the batch reactor are taken over time. The data is linearized by plotting it in integrated forms corresponding to zero, first, and second order reactions. The best fit line is used to determine n and calculate k from the slope. Analysis shows the reaction follows first order kinetics based on the straight line achieved by plotting the data as ln(CA/CAO) versus time.

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    Objective: Apparatus Required:: Experiment#3

    Uploaded by

    Fahad kamran
    35 views6 pages
    This experiment aims to determine the kinetics law parameters (reaction order n and rate constant k) of a chemical reaction between sodium hydroxide and ethyl acetate using the integral method of analysis. Conductivity readings of the batch reactor are taken over time. The data is linearized by plotting it in integrated forms corresponding to zero, first, and second order reactions. The best fit line is used to determine n and calculate k from the slope. Analysis shows the reaction follows first order kinetics based on the straight line achieved by plotting the data as ln(CA/CAO) versus time.

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    che 301

    Original Title

    cre lab 3

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    This experiment aims to determine the kinetics law parameters (reaction order n and rate constant k) of a chemical reaction between sodium hydroxide and ethyl acetate using the integral method of analysis. Conductivity readings of the batch reactor are taken over time. The data is linearized by plotting it in integrated forms corresponding to zero, first, and second order reactions. The best fit line is used to determine n and calculate k from the slope. Analysis shows the reaction follows first order kinetics based on the straight line achieved by plotting the data as ln(CA/CAO) versus time.

    Copyright:

    © All Rights Reserved
    Download as PDF, TXT or read online from Scribd
    Download as pdf or txt
    35 views6 pages

    Objective: Apparatus Required:: Experiment#3

    Uploaded by

    Fahad kamran
    This experiment aims to determine the kinetics law parameters (reaction order n and rate constant k) of a chemical reaction between sodium hydroxide and ethyl acetate using the integral method of analysis. Conductivity readings of the batch reactor are taken over time. The data is linearized by plotting it in integrated forms corresponding to zero, first, and second order reactions. The best fit line is used to determine n and calculate k from the slope. Analysis shows the reaction follows first order kinetics based on the straight line achieved by plotting the data as ln(CA/CAO) versus time.

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    © All Rights Reserved
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    Chemical Reaction Engineering Lab

    Experiment#3
    Objective:
    To determine the Kinetics Law parameters (n, k) using integral method of analysis.

    Apparatus Required:
     Batch Reactor
     Conductivity Cell

    Chemical Reaction:
     Sodium Hydroxide
     Ethyl Acetate
     Distilled Water

    Chemical Reaction:
    질፡ุ + ุ ፡፡ ุ CH3COONA + C2H5OH

    Fig-1 Batch Reactor


    Chemical Reaction Engineering Lab

    Theory:

    Integral Method of Analysis:

    This method allows one to use most or all of the experimental data in determining rate constants.
    However, one must first be certain of the reaction stoichiometry before attempting this kinetic
    analysis. In the following paragraphs, a series of linearization are presented depending on the
    reaction order. If the exact reaction order is uncertain, one may try several different
    linearizations. The best fit should occur with the linearization that is appropriate for the data (i.e.,
    indicating the correct reaction order).

    For zero order reactions, the rate is simply a constant.

    Integrating equation (1) gives:

    [ ] = [C]0 − kt

    Thus, the reaction rate constant is obtained from the slope of a plot of the molar concentration of
    "C" [Ct] versus reaction time. The intercept is, of course, the initial concentration ([C]o).

    For first order reactions, the rate is proportional to one of the reactants to the 1st power.

    Integrating equation (2) gives:

    ln[ ] = ln[ ]0 −

    Thus, the experimental data are plotted with natural log of the concentration on the y-axis and
    time on the x-axis. The reaction rate constant is simply the negative of the slope of this line, and
    the intercept is the natural log of the initial concentration.

    For second order reactions, the rate is proportional to one of the reactants to the 2nd power, or to
    two reactants, each to the 1st power. For the former case the following rate equation holds.

    Integrating equation (3) gives:


    Chemical Reaction Engineering Lab

    Thus, the experimental data are plotted as the reciprocal concentration (y-axis) versus time
    (xaxis). The reaction rate constant is simply the slope of this line, and the intercept is the
    reciprocal of the initial concentration.

    Procedure:

    1. Firstly set the rpm of peristaltic pump at 14.

    2. Make up 1L solution of 0.05M of sodium hydroxide and 0.05M of ethyl acetate.

    3. Switch ON the main power supply on the main switch of batch reactor.

    4. Set the temperature controller at 25oC.

    5. Charge the reactor with 0.5L of both reactant solutions.

    6. Adjust the conductivity meter probe inside the reactor and switch it ON for taking the
    reading of conductivity.

    7. Switch ON the reactor agitator and also adjust its rpm, note down the results on the
    interval of 3 minutes.

    8. Switch OFF the main power supply of the reactor and wash it off with distilled water

    Table-1: Kinetic law Parameters

    Sr No. T(min) CA -ln(CA/CAO) 1 / CA


    1 / CA2 - 1 / CAο2

    01 0 0.1 0 10 0

    02 2 0.065 0.431 15.38 136.69

    03 4 0.034 1.079 29.41 765.05

    04 6 0.0178 1.726 56.18 3056.167


    Chemical Reaction Engineering Lab

    05 8 0.0105 2.254 95.24 8970.29

    06 10 0.0084 2.477 119.05 14072.34

    07 12 0.0050 2.996 200 39900

    08 14 0.0035 3.352 285.71 81532.65

    09 16 0.0031 3.474 322.58 103958.27

    10 18 0.0023 3.772 434.78 188935.92

    11 20 0.0023 3.772 434.78 188935.92

    Calculation:
    Kinetic law Parameter

    Graph-1: Time vs ln(CA/CAO)

    n=1
    Slope=0.2209
    K=0.2209
    Chemical Reaction Engineering Lab

    Graph-2: Time Vs 1/CA

    n=1
    Slope=0.2209
    K=0.2209

    Graph-3: Time Vs 1/CA2-1/CAO2


    Chemical Reaction Engineering Lab

    Conclusion:
    By finishing this lab we are capable of locate out Kinetic Law parameters for a given chemical
    response of Sodium hydride (NaOH) with Ethyl acetate ( ุ ፡፡ ุ3).And capable of find
    out its slope with the help of hetero line equation and from its graph we discover that the
    instantly line occurs in first and 2d order. We discover that which order has directly line with the
    given experimental values.

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