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

Aim: To study and investigate the effect of temperature on the rate of the reaction between sodium thiosulphate and hydrochloric acid.

Extracts from this document...


VIKRAM GANESHAN 11-D CHEMISTRY HL Planning (a) Aim: To study and investigate the effect of temperature on the rate of the reaction between sodium thiosulphate and hydrochloric acid. Theory: For a reaction to take place the particles of the reactants have to collide. As particles approach each other there is repulsion between the electron clouds of the particles. In order for the reaction to occur the collision must have sufficient energy to overcome this repulsion. Frequently energy is also required to break some of the bonds in the particles before the reaction can take place. The collisions that result in a chemical reaction are known as effective collisions. In order for effective collisions to take place, a minimum amount of energy called activation energy is required which varies from reaction to reaction. Thus in order for a reaction to occur, the particles must collide and the collision must be energetically effective so as to overcome the activation energy of the reaction. The steric factor must also be taken into consideration as the collision must bring the reactive parts of the molecule into contact in the correct orientation. Thus if anything increases the collision rate, the reaction rate also increases. The rate of a chemical reaction depends on a number of factors. 1. Size of particles 2. ...read more.


7. Repeat the experiment at different temperatures. 8. Plot a graph of time against temperature. Data Collection It was observed that as soon as the contents of the two test tubes were mixed, the colour of the solution darkened and it gradually turned opaque and the cross was not viewable from the top. S.No. Beaker No. Temperature/ + 0.1?C Temperature/+ 0.1K Time / + 0.01s Reaction Rate (1/t) / +0.01s-1 1. A1 28 oC 301 135.00 s 0.007407 2. A2 38 oC 311 90.05 s 0.01105 3 A3 48 oC 321 61.10 s 0.01637 4. A4 58 oC 331 36.50 s 0.027397 5. A5 68 oC 341 22.01 s 0.045433 Data Analysis The graph for reaction rate against the temperature of the reactant mixture is given below: The hypothesis has been proved right. The time taken for the reaction to be complete decreases with increasing temperature. Evaluation The graph of the rate against temperature is a rising exponential curve, which shows that temperature is proportional to the rate of a chemical reaction and is an exponential function of the rate. The main principle on which it was based on was that in the main reaction, as sulphur is produced, it forms a dirty-blackish colloid and hence the cross below becomes invisible, thus providing a certain way to measure the end of the reaction. ...read more.


3. More accurate instruments must be used such as a burette with a better degree of accuracy for precise recordings and calculations. 4. Each time for one set of readings, It is preferred that the same person records the time after the disappearance of the cross so as to make the experiment fair as otherwise different reaction times of different people will adversely affect the experiment. Modifications Several modifications can be made to this experiment to obtain a better result. * The range of temperature could have been larger, taking into account temperatures lower than room temperature. This would enable us to judge the relation between temperature and rate of reaction more accurately. * This experiment is based upon human perception of the time taken for the cross to disappear. This could be a major area of error. An improvement could be the addition of an indicator, which could indicate the end of the reaction. * Instead of using a measuring cylinder to measure the volumes of sodium thiosulphate and water, a pipette could be used. This ensures that all the readings are taken using exactly same volumes of liquid. Conclusion Through this experiment, it is concluded that the absolute temperature is proportional to the reaction rate and the graph of reaction rate against temperature is a rising exponential curve. It was also inferred that for every 10?C rise in temperature the reaction rate doubles. 1 ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate 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 International Baccalaureate Chemistry essays

  1. Disappearing cross experiment

    of 2 M hydrochloric acid * A cross was drawn with a pen on a card and then placed on the table * The stop clock and the hydrochloric acid were placed on the table, ready for use * The conical flask, with sodium thiosulphate was then put into the

  2. What is the rate equation of the reaction between sodium thiosulphate and hydrochloric acid?

    of water /cm3 Volume of HCl /cm3 Time /s 50 0 10 61.3 40 10 10 61.9 30 20 10 66.4 15 35 10 75.4 5 45 10 121.6 Observations - As the reaction proceeds, the solution gradually becomes cloudy due to the formation of insoluble sulfur.

  1. How duration affects the rate of electrolysis in a Voltaic Cell

    the number of electrons in copper electrode, the following equation may be used:- Number of electrons = molar mass � mass of electrode (mass of one of the samples) = 65.50 � 32.08 = 2.04 Therefore, this would be the half-equation which would occur at the cathode: Cu2.04+ + 2.04e-

  2. Investigate the rate of reaction of luminol in various factors. The objective was to ...

    For example, when investigating the concentration of hydrogen peroxide, the concentration of luminol solution and the temperature must remain the same throughout the investigation. A sample has made to determine the end point of the reaction, and to give a approximation of time to the reaction.

  1. Aim: To calculate the activation energy (EA) for the reaction between Br- and BrO3- ...

    This is done by adding a limited amount of phenol and the dye methyl red to the reaction mixture, the bromine reacts very rapidly with the phenol to form tribromophenol. This is expressed in the following equation: Once all the phenol has reacted, the excess of Br2 is released by the reaction.

  2. The rate of reaction between sodium thiosulfate and hydrochloric acid

    Open the tap, let the water drain out. Repeat this step with the other 2 burettes. 2. Attach 3 burette to 3 retort stands and take care that the burettes are upright and stable. 3. Close the tap of the first burette and pour sodium thiosulfate into the burette through the funnel.

  1. What effect does the change in temperature have on the reaction rate of the ...

    To determine the frequency factor (Arrhenius Constant) and the activation energy of the reaction the following equation must be used. Where k= 1/time, A = the frequency factor, Ea= the activation energy, R = 8.314J K-1 and T = the temperature in Kelvin.

  2. Period 3 Chlorides. Aim: To study the chlorides of period 3 elements and ...

    Also since in the solid state the ions are not free to move (lack of mobility), then this is why ionic compounds do not conduct electricity in such a state. But when the bonds are broken (in the liquid/molten state), the ions are free to move and so that's why conductivity improves.

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