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

Find out the effect of acid concentration on the rate of reaction

Extracts from this document...


Coursework - Rates of Reaction By Danny Rowe In this investigation I am aiming to find out the effect of acid concentration on the rate of reaction. In a chemical reaction there are four factors that affect how quickly the reaction takes; this is also known as its reaction rate: * Temperature * Concentration * Surface Area * Catalyst The reaction I will be looking at is the reaction between magnesium (Mg) and Hydrochloric Acid (HCl) 2Mg + 2HCl -> 2MgCl + H2 I will not be looking at the effect of temperature because this variable is difficult to control, surface area is very difficult to measure and catalysts would be very expensive, therefore I have decided to do concentration as this is easy to measure and vary. To do this investigation I will get different concentrations of acid and time, using a digital stopwatch how long it takes for the acid to react with the magnesium. This will give me the reaction rate which I can incorporate into a graph and compare which other data to help me determine how acid concentration affects the reaction time. To make the experiment as safe as possible I am going to make every effort to insure that I am wearing goggles at all times and that there is no possibility of any nearby objects obstructing me or potentially making the experiment dangerous. ...read more.


To help me develop my prediction I have used various sentences from the webpage, www.chem4kids.com/files/react_rates.html. Now that I have developed a prediction based on theoretical knowledge and information from other sources I now have the ability to develop a graph displaying the likelihood of the results. The graph is below: The reason why I felt that the rate of reaction is proportional to the acid concentration is that from my understanding I feel the higher the acid concentration the faster the rate of reaction, which I have backed up with scientific evidence previously. Towards the end there is a slight bend, the reason why I have incorporated this is that I feel that it would begin to gradually level off to 0.01 seconds as I feel it would be incorrect to suggest that with a acid concentration of fifty millilitres it will take 0.01 seconds to react with the acid when at forty millilitres it takes 250 seconds. Now that I have a solid understanding of what I am going to do in the investigation and have a rather strong prediction with accompanying evidence I am now ready to begin. The results I have retrieved are below: Acid/Water (ml) Time 1 (S) Time 2 (S) Time 3 (S) Time 4 (S) Time 5 (S) Average (S) 50/0 79.8 75.0 66.6 73.8 74.4 73.92 40/10 94.2 68.4 91.8 126.6 85.2 93.24 30/20 420.6 306.0 273.0 180.6 249.6 285.96 20/30 687.0 727.8 634.8 739.8 787.8 715.44 10/40 901.8 975.6 ...read more.


and see how that makes a difference to the reaction rate. After completing this, if the shape of the line followed a similar pattern to the previous tests then this would dramatically support my evidence and prediction. The chemical equation is below 2K + 2HCl -> 2KCl + H2 The results I have retrieved from the tests are below: Acid/Water (ml) Time 1 (S) Time 2 (S) Time 3 (S) Time 4 (S) Time 5 (S) Average (S) 50/0 48.4 53.5 66.6 28.7 50.4 49.52 40/10 57.7 39.2 57.6 97.6 55.1 61.44 30/20 383.8 247.7 233.4 151.0 213.8 245.94 20/30 646.9 692.2 605.7 707.4 752.5 680.94 10/40 868.9 938.7 947.4 888.7 935.0 915.74 To make the data easier to analyse and interpret, I am going to place the data into a graph which is located below: From the graph it is evident that there is a positive correlation and that the rate of reaction increases at a relatively proportional rate to the acid concentration which is exactly what occurred in the previous experiment. The only major difference is that the overall reaction time is significantly quicker, which is almost certainly due to the fact that potassium is higher then magnesium in the reactivity series. This helps me significantly prove the below statement. From this investigation I have found out that the higher the acid concentration the quicker the reaction rate as there is more acid particles to collide with the magnesium, which I have thoroughly backed up in numerous ways. This document was downloaded from Coursework.Info - The UK's Coursework Database 1 ...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. Find out how different concentrations of HCl affect the rate of the reaction with ...

    Then wash the test tube thoroughly. 10. Clean the test tube dry with a paper towel before you repeat the experiment. 11. Repeat the experiment 3 times. 12. Clean the gas syringe with a paper towel every 2 experiments to prevent it from sticking.

  2. Investigate various ways of increasing the rate of a chemical reaction and evaluate which ...

    We shall therefore limit our investigation to the effect of three things; concentration of hydrochloric acid, temperature and surface area of calcium carbonate. Variables: There are three main types of variable; Independent (input), control and dependent variables.

  1. Rates of reactivity.

    * The concentration of any reactants will remain the same in order to conduct a fair test. * I will try to make sure that the marble chips will be of the same size, amount and mass. This is taken into consideration, as I want to keep the chips as

  2. An Investigation into the effect of Acid Concentration on the Rate of Reaction

    Taken Volume of Acid Volume of Gas produced Mass of Calcium Carbonate Surface Area pf Calcium Carbonate Light Intensity Use of a Catalyst Pressure This will then produce a picture representing the relationship between acid concentration and rate of reaction.

  1. Science Coursework

    put bags/coats out of the area where you or anyone else is working. (avoid people falling over. Especially with equipment in their hands.) 4. stand up whilst conducting the experiment. (if a chemical spills its easier to bet away. 5. walk with chemicals and equipment.

  2. Investigate, analyse and evaluate the effect on the rate of reaction of varying the ...

    results have the same variables changing and remaining constant, this way I should not get any anomalous results. I will also use pure, distilled water so there are no impurities to affect the experiment and I will take the funnel out of the burette while filling the conical flask so no drips will make my measuring inaccurate.

  1. Study the reaction kinetics and find out evidence about the mechanism between the reaction ...

    We can see if ?H is negative, hence energy lost, so the product is more stable, means the reaction would happen. Ref, 'Chemistry in context' Integrated Rate Laws The rate of reaction is proportional to the rates of change in concentrations of the reactants and products; that is, the rate is proportional to a derivative of a concentration.

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

    'Y' is multiplied by and 'S' is rate of reaction which is unknown and trying to be obtained. I predict that the higher concentrations will give off H2 faster for the reasons in the justification of hypothesis section. These higher concentrations are shown as the steepest lines in the graph

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