• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Rates of Chemical Reactions

Extracts from this document...


Introduction The rate at which a chemical reaction occurs depends on several factors: the nature of the reaction, the concentrations of the reactants, the temperature, and the presence of possible catalysts. In this experiment we will study the kinetics of the reaction between iodine and acetone in acid solution: O CH3 - C - CH3 + I2 ? CH3 - C - CH2I + H+ + I- In order to determine what affects the rate of this reaction, we will be making 4 different mixtures, keeping constant the concentration and temperature in order to determine the order of each chemical in this reaction. Objective The objective of this lab is to determine the rate of the iodination of acetone by differing the amounts of reactants, finding the rate constant (k) and the order of the reaction in terms of each of the reactants. Equipment * 4.0 M Acetone * 1.0 M HCL * 0.0050 M I2 * Distilled Water * Three 50mL Burette * Two Double Burette Clamps * Support Stand * Three small funnels * 125mL Erlenmeyer ...read more.


: I. The first mixture was 20mL of H2O and 10mL of the other three. II. Second mixture was 20mL of Acetone and 10mL of the other three. III. Third mixture was 20mL of HCL and 10mL of the other three. IV. Fourth mixture was 20mL of I2 and 10mL of the other three. 6. For each mixtures we performed two runs. Reaction Rate Data Mixture Volume of 4.0M Acetone (mL) Volume of 1.0M HCL (mL) Volume of 0.005M I2 (mL) Volume of H2O (mL) 1st Run time in seconds 2nd Run time in seconds Temp. in degrees Celsius I 10 10 10 20 218sec 209sec 26� C II 20 10 10 10 91sec 104sec 25� C III 10 20 10 10 89sec 91sec 24� C IV 10 10 20 10 385sec 365sec 25� C Determination of Reaction Orders with Respect to Acetone, H+, and I2 Mixture Acetone H+ (I2)0 Rate=(I2)0/avg.time I 0.80 M 0.20 M 0.0010 M 4.68 x 10-6 II 1.6 M 0.20 M 0.0010 M 1.03 x 10-5 III 0.80 M 0.40 M 0.0010 M 1.11 ...read more.


x 10-5 /(0.80M)1.14(0.0010M)0.18(0.40M)1.24 = 1.11 x 10-5 /.0674647592 = 1.65 x 10-4 * Rate IV: k= 5.33 x 10-6 /(0.80M)1.14(0.0020M)0.18(0.20M)1.24 = 5.33 x 10-6 /.0325607537 = 1.64 x 10-4 CONCLUSION In the iodination of acetone, we found the order of the reaction with respect to acetone and HCl and find a value for the rate constant, k. Since the concentrations of acetone and HCl were much higher than that of I2, the concentrations of acetone and HCl changed very little. Thus the rate was determined by the time needed for iodine to be used up. Since iodine has color we can easily follow changes in iodine concentration visually. The equation, rate = k(A)m(H+)n(I2)p, can be simplified to rate = k[I2]/t since the values for acetone and HCl essentially remain constant during the course of any run. In mixtures I & IV the constant rate were similar, even though the iodine doubled in mixture IV, it is still the limited reagent. Mixtures II &III were similar do to the doubling of acetone in mixture II and HCL in mixture III. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Inorganic Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related AS and A Level Inorganic Chemistry essays

  1. Peer reviewed

    Determining the concentration of acid in a given solution

    5 star(s)

    meniscus was resting on the calibration line to ensure an accurate result. If I had filled the volumetric flask up with the meniscus slightly above the calibration line, the concentration of the sodium carbonate would be slightly lower. This would mean that less acid would be needed to neutralise the

  2. Peer reviewed

    Deducing the quantity of acid in a solution

    5 star(s)

    Therefore, it is very important to ensure that we are comfortably reading it or otherwise, the results would be affected. So, to read the graduation mark of the burette, we put the equipment at a comfortable position to be read, so we could have a clear reading of the bottom of the meniscus.

  1. effects Concentration and Temperature on the Rate of Reaction

    As I have already mentioned, the rate of reaction will have approximately doubled with this rise in temperature - this is around a 100% increase. This shows that the effect of increasing collision frequency on the rate of reaction is almost negligible.

  2. Determining an Equilibrium Constant

    added /g - - - 1.04 2.95 (9) Initial amount of H2O(l) /mol - - 0.2612 0.3200 0.4306 (10) Eqm. amount of H2O(l) /mol - - 0.2323 0.2944 0.4141 (11) Equilibrium constant, Kc - - 0.1757 0.1659 0.2832 = 0.21 Precaution The deionized water used to rinse the reagent bottle and the time used for titration should be

  1. Chemistry Iodine Clock

    The rate of reaction can stay the same, it can double and the rate of reaction can also quadruple. The rate of reaction staying the same, doubling or quadrupling is called the order of reaction. Zero Order Reaction In a zero order reaction if the concentration of a reactant is doubled then the rate will not be affected, e.g.

  2. Preparation and Standardization of 0.010 M EDTA

    After the dissolution, the zinc was quantitatively transferred to a 500-mL volumetric flask. The flask was filled to the line with DI water and upended 15 times to ensure the solution was complexly dissolved. Standardization of EDTA solution. Three aliquots of standard zinc solution were prepared by carefully pipetting 10.0�0.2 mL into three 250-mL Erlenmeyer flasks using a volumetric pipette.

  1. The preparation, analysis, and reactions of an ethanedioate complex of iron

    Procedure for the reactions of the complex Oxalate Three tests tubes with our product and three with iron(III) chloride were prepared and marked correspondingly. Dilute sodium hydroxide, ammonium thiocyanate, and ammonium thiocyanate with dilute sulphuric acid were added separately into each of the three test tubes containing our product and the three containing iron(III)

  2. The Effects of Strong and Weak Acids on the Order of a Reaction.

    and Ethanoic Acid (C2H3OOH). My Experiment - Order For the order reaction, I will be using strong and weak monobasic acids to test whether the strength of the acid has any effect on the order of the reaction. As I'm using comparing strong and weak acids, I have to make

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work