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

To find the perfect acid concentration to use for an assessed practical

Extracts from this document...


Preliminary Work Aim The aim of this experiment is to find the perfect acid concentration to use for an assessed practical. Method I accurately measured 25cm? of 1M Hydrochloric Acid and poured into a beaker. I dropped 1cm Magnesium into the Hydrochloric Acid and timed how long the Magnesium took to react with the Hydrochloric Acid. I did this over again with the same quantity of Magnesium and Hydrochloric Acid, but changed the acid concentration (the variable). The concentrations, which I used, were: 1.0M, 1.5M, 2.0M, 2.5M and 3.0M. Results: Acid Concentration/M Time/S Rate/cms-1 1.0M 57.45s 0.0174 1.5M 40.38s 0.0274 2.0M 40.00s 0.0250 2.5M 08.64s 0.1157 3.0M 48.00s 0.0208 Conclusion I think that a Hydrochloric Acid concentration of 1M would be most suitable for the assessed practical. I believe this because it had an appropriate rate of reaction at room temperature, and therefore should have a good rate of reaction when heated. I think 2.5M would be the worst choice of acid concentration because the time would be too little, especially when heated. Investigate The Factors That Affect The Rate of Reaction Between Magnesium and Hydrochloric Acid Depending on certain factors (or variables) the rate of reaction will either increase or decrease. The factors that may affect the rate of reaction are as follows: * Temperature * Amount of Hydrochloric Acid * Mass of Magnesium * Surface area of Magnesium * Concentration of Hydrochloric Acid * Pressure * Catalyst . ...read more.


A catalyst, which slows down a reaction, is called a negative catalyst. Catalysts speed up reactions by offering a 'alternative' pathway for the reaction, i.e. one that has much lower activation energy. More collisions will, therefore, have enough energy for this new pathway Prediction I predict that when using prediction as a variable the collision theory will be correctly applied to my results. I think this because I have good evidence (Boltzman distribution curve). I also believe that it makes sense that the higher the temperature, the more energy the particles will have to collide and react successfully. I predict that the Q10 theory will be relative to my experiment a great deal and that it will work. The Q10 theory is that for every 10?C the temperature goes up the rate of reaction is doubled. The rate of reaction will increase when temperature and surface area of Magnesium is increased and acid concentration of Hydrochloric Acid is lowered. Method 1. Collect equipment: - Magnesium, 1M Hydrochloric Acid, Thermometer Test tube, Pipette, Vernier Callipers, Kettle, Water, Emery paper (This may affect the rate of reaction when surface area of Magnesium is applied is that Magnesium oxide (Magnesium Oxide) can affect the surface area of Magnesium. When oxygen reacts with the Magnesium, Magnesium oxide is formed which can 'eat away' slightly at the Magnesium. ...read more.


I don't think any of my results were particularly odd, but if you see my graph the 30?C result looks slightly out of place on the line of best fit. Apart from this my results were mostly constant and steady. I repeated all my results three times because if a odd result did occur I could compare it to the two other results and maybe do it again. In some of my repeats there were a few slightly odd results, but nothing too major to make a difference. If I were to do this experiment again I would more research in the form of preliminary work and I would use another variable as well as temperature, to see if temperature is what affects the rate of reaction the most I would also repeat the results at least six times to get a better average. If I were to do any further work on this experiment, I would do more research into how Hydrochloric Acid and Magnesium react with and without temperature changes, I would see if the Q10 theory could be proved with another experiment and compare the two experiments. I would also improve the amount of gas is collected to do this I would use a video camera to allow you to work out the volume of gas more accurately every 20 seconds as you could use the freeze-frame facility. ?? ?? ?? ?? Emma Dovaston 11GG ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Patterns of Behaviour 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 GCSE Patterns of Behaviour essays

  1. How does changing the concentration of the Hydrochloric acid affect it reactions with Magnesium?

    To reduce the heat produced from the experiment a water bath will be used throughout the experiment. This will control the temperature. Solutions: I have decided to use 1 mole for the concentration of acid. This is because 2 moles was too reactive and there were not enough results to collect due to the rapid rate of reaction.

  2. How does changing the concentration of hydrochloric acid affect its rate of reaction with ...

    So at a higher concentration of hydrochloric acid, the rate of reaction will be much faster compared to the rate with a small concentration of hydrochloric acid. I predict that the rate at which hydrogen is being produced will be much quicker in the highly concentrated solutions, which means that there is faster rate of reaction between the reactants.

  1. Investigating the affect of concentration on the rate of reaction between magnesium and hydrochloric ...

    This is because in order for particles to react they must collide with enough energy and in the correct orientation for bonds to be broken. This is because for a chemical reaction to take place, some bonds in the reactants must be broken. This is shown in the diagrams below.

  2. Magnesium Oxide

    mat so that there are no burns around the area or the possibility of fire. The crucible and lid would be placed above the pipe-clay triangle so that the heat would reach the crucible in the right place. The tripod would be used to keep the crucible and lid above the Bunsen burner at the right distance.

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