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

Investigate a factor which affects the rates of reaction between magnesium ribbon and hydrochloric acid.

Extracts from this document...

Introduction

INVESTIGATING REACTION RATES Aim: To investigate a factor which affects the rates of reaction between magnesium ribbon and hydrochloric acid. Background Knowledge The rate of a chemical reaction is the speed that the reaction takes to finish. For a chemical reaction to take place reagent particles must collide with each other and the collision must have enough energy if a reaction is to take place. This energy is called the activation energy. There are several things that can be done to speed up the reaction, which increase the rate. * Temperature Increasing the temperature increases the energy particles possesses, and so more particles possess the minimum energy (activation energy) and so reaction is faster. * Concentration of acid There are more reactant particles at a higher concentration in a volume. Therefore there is more chance of collision. Dilute solution Concentrated Solution * Surface Area Increasing S.A increasing rate of reaction. This is because smaller particles have a higher total surface area exposed for reaction and therefore more collisions occur, making the rate of reaction faster. Magnesium Ribbon Powdered Magnesium * Catalysts they provide a different pathway with a lower activation and so the reaction speeds up the reaction without being chemically changed itself. The diagram above shows the energy level diagram for a reaction both with and without a catalyst. ...read more.

Middle

I filled the 250ml beakers, one with the acid and one with distilled water, and brought it to my desk, this prevented me from having to go back and forth across the class to collect more. Method 1. Collect all the apparatus in the list above. 2. Put on your safety goggles 3. Collect 64cm of Magnesium ribbon and using scissors cut it into 16 separate pieces, each measuring 4cm long. 4. Pour the acid and water into the separate 250ml beaker and bring it over to your desk. 5. Then measure out 50cm3 of acid use the 25ml measuring cylinder (using it twice) and pour this into the 50ml beaker. 6. Drop the 4cm strip of magnesium into the beaker and immediately start the stopwatch. 7. Hold the ribbon under the surface of the acid with the stirring rod, as to increase the surface area in contact with the acid, until dissolved. 8. As soon as the magnesium dissolved, stop the stopwatch and record the time in your results table. Rinse the beaker. 9. Now measure out 45cm3 of acid, again using the 25ml measuring cylinder (twice, this is so increase the accuracy) and 5cm3 of distilled water (using the second measuring cylinder) and pour both the acid and water into the 50ml beaker again. ...read more.

Conclusion

Evaluation Overall, I think that my experiment went well. The method was simple and easy to follow and I didn't encounter any problems whilst carrying out the experiment. It also proved that my prediction based on my background scientific knowledge was right. Therefore my method does work and give good results. However, as human intervention is involved when starting and stopping the stopwatch my results may not be completely accurate. There are several ways I could change my experiment in order to make it more accurate. For example I could collect the volume of gas given off, or I could have used a burette. However, the best way to increase volume accuracy would be to use a pipette, as it is accurate to 0.02 cm3. I used a wide range of different concentrations and obtained a variety of good results. They all follow the same general trend although I have on anomalous results at 60% concentration of the acid. My results prove that when the concentration of the solution is increased, the rate of reaction is also increased. As I have already mentioned above, another way to carry out the experiment would be to measure the amount of hydrogen gas given off during the reaction. You could do this by following the same method but this time collect the volume of hydrogen gas given off in a gas syringe. Below is a diagram of the new apparatus needed. ...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. Marked by a teacher

    In this project I am going to investigate rates of reaction of an indigestion ...

    3 star(s)

    Plan NB. Although this is the final plan for the actual experiments, a lot of the volumes and other measurements weren't worked out until the preliminary experiments were done (see pages 6, 7 and 8). In the preliminary experiment section I have specified the areas that I was investigating.

  2. Investigating the rate of reaction between Magnesium Ribbon and Hydrochloric Acid.

    My prediction has therefore been proved right. If I then plot these results of average rate of reaction against time a pattern might emerge. When I drew the line of best fit, I saw that if you double the concentration then the rate of reaction doubles. It is a positive correlation in direct proportion.

  1. Experiment to investigate how changing the concentration of hydrochloric acid affects the rate of ...

    The graph clearly supports my prediction. However, on this graph as well there is an anomaly. I have explained earlier the cause of this anomaly and why I should ignore it. In spite of the anomaly, there is a strong pattern in my graph suggesting that my prediction is correct.

  2. Rate of reaction of hydrochloric acid and mangesium ribbon.

    I am saying this because of the collision theory. The higher the concentration of acid then the higher the number of acid particles present per 100cm3 of acid. This means that there will be more collisions per second, which means there will be more successful collisions per second, so the rate of reaction will increase.

  1. Free essay

    Magnesium Ribbon

    to occur and when these collisions occur, there is more chance that the collision will lead to a reaction. The particles will collide more often and thus the rate at which the product is being formed will also increase. This is because the amount of energy is more likely to

  2. Investigating the varying rates of reaction between Hydrochloric Acid and Magnesium ribbon.

    This idea, called particle theory is illustrated below. Hcl Molecule. Mg Molecule. In the diagram on the left there are 3 of Each molecule. In the diagram on the right The amount of Hcl molecules has been Doubled so there are twice as many Collisions and the reaction time is halved.

  1. Rate of reaction of hydrochloric acid and mangesium ribbon.

    conical flask, the weight change will not be very big, but there will be one. How long the magnesium takes to dissolve I could measure the length of time it takes for the magnesium to dissolve. The only problem with recording my experiment this way is that I could only

  2. Free essay

    Close Your Eyes

    *Danny* Woohoo! She's coming round mine tomorrow. Guess I'd better plan my next move. "What new song?" Tom asked me suspiciously as I entered the front room. "He hasn't got one. It's just cos he fancy's her and wants to snatch her up before someone her own age does.

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