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

Using different concentrations To speed up the rate of reaction.

Extracts from this document...

Introduction

Using different concentrations To speed up the rate of reaction Introduction In this investigation I am going to look at the different factors that affect the rate of reaction. The factor that I am going to investigate is the concentration of the acid used, which in this case is Hydrochloric acid (HCL). The different factors that affect the rate of reaction are: > Temperature > Concentration of acid > Surface area of magnesium > Catalyst > Pressure Rates of reaction means how fast a chemical reaction takes place. During a chemical reaction many changes may take place, some of these changes are obvious: e.g. the solution may change colour. The less obvious changes are: > Change in mass > Volume of gas made > PH > Temperature "Bob McDuell GCSE chemistry" Temperature Temperature can affect how fast a reaction takes place. When the temperature is increased the particles move faster as they have more KINETIC ENERGY. The faster the particles move the are more successful collisions, there are E.g. if you increase the temperature by 10`C the rate of reaction will double "Bob McDuell, GCSE Chemistry" Concentration If the acid has a high concentration the more likely it is that there will be more collisions. There will be more collisions, as there are more particles of the reactant in the solution. ...read more.

Middle

used I am going to change the following things in my experiment: > Concentration of acid I am going to repeat this experiment four times so that I can obtain accurate results. I am going to use five different concentrations of acid in my experiment. Fair test To make this experiment a fair test I will: > Amount of magnesium ribbon used > Collect the same amount of gas > Use the same volume of acid all the time Apparatus/ diagram For this experiment you will need: > Magnesium ribbon 0.15 grams each time > Hydrochloric acid up to 2 moles > Water (to dilute acid) > Pipette > Measuring cylinder - 35CM3 > Gas syringe > Stop watch > Clamp > Conical flask > Safety goggles Method > Collect apparatus > Set up as shown above > Collect magnesium ribbon 0.15g > Measure out 25 cm3 of HCL acid using a measuring cylinder (change concentration as appropriate) The concentrations that I am going to use are: > 2 molar > 1.66 molar > 1.34 molar > 1 molar > 0.66 molar (you have to change the concentration of the acid by diluting the acid with water) > Make sure that you are wearing safety goggles > Place acid into flask > Place magnesium ribbon in to flask > Quickly place bung onto flask > Check that the bung is securely on, and there are no gaps > Start timer quickly ...read more.

Conclusion

My graph doesn't prove this theory correct, but there were fairly accurate compared to the equipment I had available. I still some anomalous results, this may be due to change in environment or inaccurate readings. Evaluation I think that my method was correct, as my experiments did run smoothly. If I could do the experiment again I would do all the experiments in one day, so that there wouldn't be a change in environment. The accuracy of my experiment was good in comparison to the equipment we had available. One thing that should be improved on was the time period it took for us to place the bung on the flask, this would have effected the time taken to produce 50cm3 of hydrogen gas. Another reason for these anomalous results is that the concentration of the acid could have been wrong. Another possible reason is that when the flask was washed it may have been washed with too hot or too cold water, which would have changed one of the variables I was keeping the same in my experiment. As you can see from my results table my results were constant throughout the repeats of the experiment. If I could do the experiment again I would have repeated it again to get a more accurate average. Overall I think that my experiment went well, and that I obtained accurate results. Diagram Komal Patel 11GS Chemistry C/W ...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

    For my experiment I am finding out the effects on the reaction rate when ...

    3 star(s)

    conical flask and that you are a safe distance away from the conical flask. My preliminary results, with the time taken converted into the reaction rate for each trial. Trial1 Trial 2 Trial 3 GRAPHS TRIALS 1, 2 and 3 Method WEAR EYE PROTECTION!!!

  2. Marked by a teacher

    To monitor the rate of reaction we measure how a product changes with ...

    Usually, a rise of 10OC will double the rate of reaction. Chemical reactions take place by chance. Particles need to collide with enough velocity so that they react. As the temperature is increased the particles move faster since they have more energy.

  1. Determine the rate equation for the reaction of hydrochloric acid with magnesium metal, and ...

    concentration is: Rate = 2.67�[HCl(aq)]2 A possible pathway for the reaction is proposed on the Nuffield Advancing Chemistry website2. For the reaction to occur, first the hydrogen ions need to reach the surface of the magnesium solid. If the kinetic energy of the particles is great enough, an electron will leave the magnesium atom and reduce H+ to H.

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

    The initial rate of reaction increase as the concentration of the acid increases 2. There is a fourfold increase in the rate of reaction as the concentration increases 3. As the concentration doubles the initial rate of reaction is approximately squared My original prediction was that the initial rate of reaction would double as the concentration doubles.

  1. Rates of reactions between HCL and magnesium ribbon.

    have to make sure that I keep the following factors the same:- volume of acid used (cubic centimetres), surface area of the magnesium, length of magnesium. I will also have to make sure that the gas syringe is correctly connected and that it is placed quickly and tightly enough so that no hydrogen gas escapes.

  2. Investigating the Rate of Reaction Between Hydrochloric Acid (Hcl) and Magnesium (Mg).

    If my memory serves me correctly I distinctly remember doing both the first and second attempts of the 200C investigation on the same day, and not doing any other temperatures. This could easily mean that part of the apparatus was faulty.

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

    they will begin to bounce off each other causing the rate not to increase. Moles calculations Mg + H2SO4 MgSO4 + H2 Mole ratio 1 : 1 : 1 : 1 Info 100cm3 of H2 Moles = 100 = 0.00417 24000 We use mole ratio 1:1; therefore we need 0.00416

  2. The aim of this investigation is to find out how the different concentrations of ...

    PLAN OF THE EXPERIMENTS In this investigation adding different amounts of water to the acid would change the concentration of hydrochloric acid the independent variable would change the concentration levels of hydrochloric acid. At each concentration level the time the dependant variable it takes the magnesium strip to disappear would

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