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

Investigate the factors that effect the rate of the reactions between magnesium and acid.

Extracts from this document...

Introduction

Investigate the factors that effect the rate of the reactions between magnesium and acid. Aim: To find out what factors effect the rate of reactions between magnesium and acid Introduction: During any chemical reaction the concentrations of the reactants decrease and the concentration of products increase with time. The rate of reaction (reaction velocity) may be defined as the rate of change of concentration of a stated reactant or product. The rate of a reaction is found by measuring the amount of a reactant used up per unit of time or the amount of a product produced per unit of time. A reaction can be made to go faster or slower by changing a number of factors. In order for a reaction to occur it is necessary that: particles must collide with each other and the collision must have enough energy. If this happens the original bonds are broken and new bonds are formed - so that new products are formed. Successful collisions (those with sufficient energy) can be increased (or decreased) by a number of factors. In this experiment the factor which I will be investigating is the concentration of hydrochloric acid which would be measured in molars. Key Variables: The factors which could affect my experiment are; 1. If the temperature were to increase the rate of the reaction would also increase. ...read more.

Middle

I will also start the concentration from 1.0 molar because anything below would not show much of a result. In the preliminary experiments I noticed that as the concentration is increased the rate of the reaction will also increase. I expect the same thing to happen in this experiment. Apparatus * Strip of magnesium * 20cm� of Hydrochloric acid * conical flask * trough * measuring cylinder * delivery tube * ruler * stopclock Method: 1. First of all I will collect all equipment and measure how concentrated the hydrochloric acid should be by first using 1.0 molars. 2. Then I shall put the Hydrochloric acid in the conical flask 3. I then will fill a trough with water and put the conical flask into it and then fill another trough with water and fill the measuring cylinder with water to the top and quickly put it into the water 4. Then I will put the delivery tube underneath the measuring cylinder 5. I will add the magnesium to the hydrochloric acid and straight away start the stop clock 6. I will do this experiment a number of times increasing the concentration of the hydrochloric acid by 0.2 molar. Safety: To ensure that the experiment will be safe I will wear goggles at all times when handling the experiment and be careful not to spill any hydrochloric acid or water. ...read more.

Conclusion

So 2cm would give the most reliable results. The variable which I investigated in this experiment was the concentration of the hydrochloric acid and I found out that as I increased the concentration of the hydrochloric acid the amount of gas produced increased and so the rate of the reaction increased. This is exactly what I had predicted and this is because of the collision theory. I controlled the temperature variable because I knew that after each experiment if I had not stopped the temperature from increasing the rate of the reaction would of increased because of this as well and so my results would have been unreliable. I controlled the temperature by placing the conical flask in cold water during the experiment so that no extra heat would be added to the results. Evaluation: I think that enough data was collected for definite results because the experiment was carried out with 5 different concentrations and done 3 times with each concentration. The results do support the collision theory so I think that they are good. I don't think any of the results do not fit the pattern because as the concentration increased the amount of gas produced in the first 10 seconds would also increase but in each concentration the amount of gas produced by 60 seconds was always around 20 grams. ...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?

    it will effect the rate of reaction between the reactants, either by speeding it up if the temperature rises because the particles move faster and travel a greater distance in a given time and so will be involved in more collisions.

  2. Exothermic and endothermic reactions

    Examiner's Note Well done. Look out for questions with the word affects. There will usually be a mark for stating whether the rate increases or decreases. Question 2 What is meant by the term 'catalyst'? The Answer A substance which increases the rate of reaction but does not get used up in the reaction.

  1. Investigating the Effect of Different Concentration Of Acid Rain On The Rate Of Reaction ...

    mass of magnesium strips would quite obviously directly affect the surface area of the magnesium strips causing the reaction to have other factors affecting the rate of reaction which is undesired and will make the results incomparable. For this reason the mass of marble chips will be kept constant at three grams.

  2. 'Investigating factors that affect the rate of chemical reactions.'

    This increases the number of useful collisions. The reaction between calcium carbonate and hydrochloric acid in solution is a reaction that occurs at a moderate speed. No catalyst is necessary for this reaction to proceed, and it occurs at room temperature.

  1. What factors effect the rate of a chemical reaction?

    � Concentration of solvent (dilute hydrochloric acid) � Amount of reactants (9-12mm size marble chip and 50cm3 of hydrochloric acid) � Catalyst (no catalyst will be involved) A fair test will also require the experiment to be repeated several times at each temperature for reliable results Plan I plan to use a range of temperatures from 20�C to 70�C increasing by 10�C for each test.

  2. Safety- must always wear safety glasses and we should be very careful not to ...

    To get the best results I need to use the equipment in the best possible way. Results Evaluating Evidence I think that the experiment went very well. This is because I got all the results that I wanted and they look very good.

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