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

The effect of concentration on the reaction rate:

Extracts from this document...

Introduction

The effect of concentration on the reaction rate: I) Aim: Observe the effect of concentration on the reaction rate. II) List of equipment: - 155 cm3 of sodium thiosulphate solution - 150 cm3 of water - 25 cm3 of hydrochloric acid - flask - cylinder - timer - safety goggles - lab coat - a paper with a black cross on it III) ...read more.

Middle

* Then we redo the processes with different concentration of sodium thiosulphate solution by adding water. IV) The table of results: Volume of sodium thiosulphate solution (cm3) Volume of water (cm3) Time taken for the cross to disappear (s) Concentration of the sodium thiosulphate solution (g/dm3) Rate of the reaction (/s) 50 0 25 40 1/25 = 4.00*10-2 40 10 30 32 1/30 = 3.30*10-2 30 20 38 24 1/38 = 2.60*10-2 20 30 65 16 1/65 = 1.55*10-2 10 40 140 8 1/140 = 7.15*10-3 5 45 334 4 1/334 = 3.00*10-3 V) ...read more.

Conclusion

The graph shows that if you double the concentration it will double the rate of reaction. It may happen like that, but the relationship may well be more complicated. Conclusion: This reaction involves collision between two different types of molecules: molecules of hydrochloric acid and molecules of sodium thiosulphate solution. In order for any reaction to happen, those particles must first collide. If the concentration is higher, the chances of collision are greater and the reaction happens quickly. ...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. Investigate the rate of reaction of luminol in various factors. The objective was to ...

    5.61 18.86 25.17 38.20 44.13 48.47 53.41 58.86 64.57 70.74 Anomalous Result C. Investigation: rate of reaction in different temperature Temperature (�C) 0 15 30 40 50 60 70 80 Time 1 (s) 10.40 65.31 48.97 31.25 54.34 75.22 42.56 13.03 Time 2 (s)

  2. Aim: To study and investigate the effect of temperature on the rate of ...

    Place the conical flask in a water bath and heat the contents to a particular temperature. Record the temperature. 3. Place the flask on a white tile which is marked with a cross. 4. Immediately, add 5cm3 of hydrochloric acid to the heated solution.

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

    concentration of 0.1 mol dm-3 of sodium thiosulphate: (49.7+55.4)/2 = 52.55 s Average time taken by solution for different sodium thiosulphate concentrations: Concentration of Na2S2O3 /mol dm-3 Average time taken by solution /s 0.10 52.6 0.08 69.0 0.06 95.1 0.03 302.5 0.01 979.5 Average time taken by solution for different

  2. Chemistry extended essay - investigate the effect of 2-bromo-2-methyl propane concentration and temperature of ...

    Ln [Rcl] 0 = - Kt - 2.303 Log [Rcl] 0 = - Kt [Rcl] t 2.303 Log [Rcl] 0 = Kt [Rcl] t Where [Rcl] 0: is the molar concentration at time t = 0 [Rcl] t: is the molar concentration at time t = t Two methods to

  1. 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.

  2. Rate of Reaction sodium thiosulphate

    (note: the solute particles in solutions have the smallest particle size possible. and so solutions react fastest) Collisions occur at the surface of particles. The larger the particle size the smaller the surface area and the fewer collisions can occur.

  1. Reaction Rate

    * The same mass of Magnesium (Mg) ribbon to be reacted with the H2SO4 solution (0.05g). The laboratory technician will keep this constant beforehand, as they will provide us with the pre-cut ribbons for our experiment. This mass has been chosen, as it is a sufficient for a distinct reaction to be witnessed in a suitable period of time.

  2. Determining the of the Effect of the Concentration of Na2S2O3 on the Rate of ...

    Calculations To calculate the concentration of the Na2S2O3 in each trial, we use the equation: . As for both trials the volumes are all identical, we can simply calculate the concentrations for the first trial, and use them for the second.

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