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

Factors affecting the rate of a reaction.

Extracts from this document...


Science Coursework Factors Affecting the Rate Of A Reaction Aim: The aim of our experiment is to find out the effect of Hydrochloric acid concentration on rate of reaction with magnesium. What I Already Know: I already know that when hydrochloric acid reacts with magnesium it creates magnesium chloride and gives off hydrogen gas. I also know due to my preliminary experiments that this is an exothermic reaction, which means that heat is given out during the reaction. Volume of acid (cm3) Temperature increase after the reaction (degrees C) 10 15 20 14 40 7 Using these results I can choose the volume of acid I am going to use. If I used 10cm3 the temperature given off might affect my results. From the results I have collected I can observe that I should use between 25cm3 and 40cm3 in order to avoid the heat affecting my reaction. Also due to this experiment I have discovered that as you increase the volume of the acid in this reaction the amount of heat given off is shared amongst the bigger volume therefore affecting the results of my reaction less. ...read more.


We know any less than this will result in a temperature rise that may affect our results. First we will set up our apparatus (see diagram). Then we will do the experiment using different concentrations of acid with a range of 0.5 molar to 1.5 molar. We will measure the amount of hydrogen gas produced every 10 seconds to find the rare of reaction. The strip of magnesium we use will be 2cm long each time. We will repeat our readings twice In order to attain an average and hopefully avoid any anomalies that may occur. Diagram: Equipment: Conical flask Hydrochloric acid Stopwatch Magnesium strips Measuring cylinder Ruler Empty ice cream tub Ruber tube Prediction: I predict that as we increase the concentration of the acid, the time taken for the reaction to finish will decrease. As a result of this the rate of reaction will increase. I believe it will do this because as we increase the concentration of the acid the more acid particles there are to the same volume and less water particles there are, therefore more acid particles will be moving around in the reaction increasing the chance of successful collisions between hydrochloric acid and magnesium particles. ...read more.


16 16 1.5 4.5 14.5 15 15.5 15.5 15.5 15.5 15.5 15.5 15.5 15.5 15.5 Conclusion: From the graph and my results table i can see that my prediction was proved right .This is due to the fact that i stated that the highest concentration Hydrochloric Acid (1.5M) would have the fastest reaction rate(4.5 cm3 produced in 10 s) whereas the lowest concentration of Hydrochloric Acid (0.5M) would have the slowest reaction rate (1 cm3 produced in 60 s)which were both shown to be correct. However this is not including water which didn't have any effect on the magnesium whatsoever.This is because in order for any reaction to occur, particles of both substances must first collide. In a solution with a higher concentration there is a larger amount of particles to react thus allowing for more successful collisions and a higher collision frequency to occur. As reactions rely on successful collisions occuring, a higher collision frequency leads to a faster reaction rate. Furthermore as the number of water particles decreases there is becomes a smaller chance of the acid particles becoming obstructed by the water particles thus giving them more possibilities to collide with the magnesium. ...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 Aqueous 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 GCSE Aqueous Chemistry essays

  1. To investigate the factors affecting neutralisation.

    This time I will also use a polystyrene cup to hold the acid and alkali mixture. This is because polystyrene is an insulator and so less heat will be lost making my experiment more accurate. To record the temperature changes I will use data logging equipment to record the temperature every 10 seconds.

  2. See how different concentrations of Hydrochloric acid change the rate of reaction with a ...

    I also used these quantities of chemicals because it has kept the temperature increase to a minimum. Method 1st Experiment 1. Put on safety goggles 2. Collect all the equipment required to do the experiment and set them up, which includes magnesium, 5 different concentrations of hydrochloric acid, 5 test tubes, test tube rack, measuring cylinder and stop clock 3.

  1. Rates of Reaction

    In addition to this the marble chips took a considerable amount of time to weigh which again prolonged the experiment and due to these reasons I will not be using this method due to its unreliability and the time consumption.

  2. An investigation into the factors affecting the rate of reaction of indigestions tablets with ...

    I thought I should test between 20% and 60% as the spacing between each different concentration can be constant (10cm3) and it allows us to look at a broad range of concentrations from low - quite high. Method for Concentration preliminary, -I took 5 different beakers and filled them with

  1. Investigate one of the factors that effects the rate of reaction between Magnesium and ...

    ml of 1M Hydrochloric Acid + 5 ml of 2M Hydrochloric Acid 1.6M = 2 ml of Water + 8 ml of 2M Hydrochloric Acid 2.0M = 10 ml of 2M Hydrochloric Acid By using these amounts of the different acids and water, the different concentrations can be formed.

  2. Rate of Reaction

    Catalysts though are non-reactants. Stirring - The effect of stirring increases the rate of reaction because it causes the particles to move quicker and so each collision between the particles becomes more violent. As the particles move around faster they gain more energy also which in turn helps to make the collision much more vigorous.

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