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

All chemical reactions involve reactants, which when mixed may cause a chemical reaction which will make products. In my case the reactants are hydrochloric acid and magnesium ribbon.

Extracts from this document...


Introduction All chemical reactions involve reactants, which when mixed may cause a chemical reaction which will make products. In my case the reactants are hydrochloric acid and magnesium ribbon. In the reaction between hydrochloric acid and magnesium ribbon, the hydrochloric acid will dissolve the magnesium and produce hydrogen gas. The chemical reaction takes place when the magnesium ribbon is dropped into the hydrochloric acid. The products that are formed during this reaction are hydrogen gas and magnesium chloride. The formula equation for this experiment is: Mg + 2HCl ? MgCl2 + H2 Magnesium + Hydrochloric acid ? Magnesium Chloride + Hydrogen Depending on certain factors the rate that this reaction will take place will either increase or decrease. The factors that may affect the rate of reaction are as follows: � Temperature of the Hydrochloric Acid � Mass of the Magnesium Ribbon used � Concentration of the Hydrochloric acid � Surface area of the Magnesium Ribbon used All of these factors will change the rate of reaction because of the Collision Theory. Factors The factors that could affect the rate of reaction of my experiment are as follows: � Concentration of the acid � Temperature of the acid � Surface area of the magnesium � Type of acid used . ...read more.


I will then start the stop clock and record the volume of gas evolved every 10 seconds for 160 seconds. I am measuring the initial reaction not the average. Fair Test In order to keep my experiment a fair test I will have to make sure that I keep the following factors the same: � Volume of acid used (cubic centimeters) � Surface area of the magnesium � Length of magnesium I will also need to clean the magnesium to get rid of unwanted chemicals. The apparatus and chemicals used during my experiment are as follows: Chemicals - 1.5g magnesium ribbon - 0.3M hydrochloric acid - 0.4M hydrochloric acid - 1.5M hydrochloric acid - 0.6M hydrochloric acid - 0.7M hydrochloric acid - Distilled water Apparatus � Measuring cylinder � Conical flask � Safety goggles � Test tubes � Thermometer Safety The things that I will need to do to keep my experiment a safe one for myself and other students around me are as follows: � Wear safety goggles as I am using concentrated hydrochloric acid � Care in using glassware since it is sharp when broken and can cut skin � Safe disposal of acid Method 1. Put on safety goggles 2. ...read more.


However I also said in my prediction that if I doubled the concentration from 0.3M to 0.6M hydrochloric acid then the rate of reaction will also double. I have discovered that this is not the case. As you can see from this table as the concentration doubles then the rate of reaction approximately quadruples. My graph also shows that as the concentration doubles, then the initial rate of reaction approximately quadruples. I therefore conclude that: The initial rate of reaction increases as the concentration of the acid increases. My original prediction was that the initial rate of reaction would double as the concentration doubles. This was incorrect because it was not based on experimental evidence. Evaluation I believe this test was successful enough to show my prediction was correct, but there was still room for improvement. A factor which could have harmed my results was, when I had to quickly place the rubber bung on the conical flask, this meant that different amount of gas could escape quickly. The length of magnesium could have made a difference, it was very hard to keep all the pieces the same size because the magnesium ribbon was different widths and lengths. Some of the magnesium had already started reacting before it went into the flask because, although we had cleaned it there were still some Hydrochloric acid on our hand and desks. Rates of Reaction GCSE COURSEWORK ...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. Investigating the rate of reaction between Magnesium Ribbon and Hydrochloric Acid.

    64 190 63 63 71 66 195 64 64 73 67 200 66 66 74 69 205 68 67 75 70 210 69 68 76 71 215 70 69 78 72 220 72 70 79 74 225 73 70 81 75 230 75 71 82 76 235 76 72 83

  2. How does changing the concentration of the Hydrochloric acid affect it reactions with Magnesium?

    I used 5 different strengths of hydrochloric acid. These strengths would determine the rates of reactions. Solution Moles Water H2O (cm3) Hydrochloric acid HCL (cm3) Magnesium ribbon (cm) 1 1m 40 cm3 10 cm3 30cm 2 1m 30 cm3 20 cm3 30cm 3 1m 20 cm3 30 cm3 30cm 4

  1. Investigating Factors Affecting the Rate of a Chemical Reaction

    There is no anomalousness and the average time taken for the reaction descends, as the concentration increases at a positive correlation as I predicted. There is a decrease of almost 242 seconds from the starting concentration (0.03moles/dm3) to the finishing one (0.15moles/dm3).

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

    Ways that I could record my experiment There are several way which I could record my experiment. The possible ways are as follows: Amount of gas evolved I could use a gas syringe to collect the gas that will evolve from my experiment.

  1. Rates of reactions between HCL and magnesium ribbon.

    concentration increases because the graph has it's largest gradient or it is steepest at this point. When the graph was made into 1/time the result should have been a straight line graph but it did not turn out this way even though concentration~1/time.

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

    Finding 4). The fact that neither temperatures match up is confusing but not unexplainable. The important number to keep in mind with the experiment is the final volume of gas formed, and those normally stay to within 3cm3 of each other. What happens during the reaction is a different matter.

  1. Free essay

    Magnesium Ribbon

    An example of a catalyst: Hydrogen peroxide decomposes to form water and oxygen gas: Hydrogen peroxide -> water + oxygen This reaction only occurs very slowly and it would take 500 days to produce 50 cm3 of oxygen. However by adding the compound manganese oxide that acts as a catalyst

  2. Exothermic and endothermic reactions

    Special trays collect the condensed liquid and it runs off in pipes. * Hydrocarbons with high boiling points condense first, low down the tower. * Hydrocarbons with low boiling points can get all the way to the top before they condense.

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