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

Rate of Reaction between Hydrochloric Acid and Magnesium Ribbon.

Extracts from this document...


Rate of Reaction between Hydrochloric Acid and Magnesium Ribbon In this experiment I am going react magnesium ribbon with hydrochloric acid. During this reaction the hydrochloric acid will dissolve the magnesium ribbon and produce hydrogen gas. Magnesium with react with hydrochloric acid because it is higher in the reactivity than hydrogen. When these two react a displacement reaction will take place and the magnesium will take the place of hydrogen in hydrochloric acid forming magnesium chloride and hydrogen gas. Variables * Concentration of acid - this will affect the rate of reaction because if there is a higher concentration of acid per 50cm�. Thus meaning more collision per second and so more successful collisions. * Surface area of magnesium ribbon - the greater the surface area of magnesium ribbon the bigger the area that the acid has to collide with. This means that bigger surface area will mean more collisions per second so more successful collisions. * Temperature or acid - if the temperature of the acid is increased the particles will move with more energy. ...read more.


This is because there are twice as many particles so there is twice as many chance of a successful reaction. This means that the rate of reaction will increase so that it is twice as quick. Plan For this experiment I am choosing a set size for the magnesium ribbon to be. I have chosen 1cm�. This will ensure that it is a fair test throughout. I have also made sure that my concentration of acid and water both add up to 50cm�. This will also make sure that it is a fair test. I will now choose concentrations of hydrochloric acid to use. To change the concentration I will add distilled water. I used a measuring cylinder to accurately measure out the concentrations needed. I will now pour them into a conical flask. The magnesium is now added. Using a stop watch I timed from when the magnesium ribbon landed in the hydrochloric acid until there was no magnesium left to see. ...read more.


Evaluation From my results and conclusion I think that my results are accurate. I can say this because there are no anomalous results. During my testing I could have repeated each concentration more times. This could have helped to get more varied results and also find a more accurate final reading from the average. My results certainly showed that as the concentration of acid is increased so does the rate of reaction. No results disagree with this statement. There is no real pattern in my results. The only pattern is that when the concentration of acid is increased so is the rate of reaction. If I wanted to see if this pattern continued I could change the concentration and use a lot more that range from a very low amount of acid to pure acid as I used. To see what affect the rate of reaction you could do an experiment for each variable and use this and compare the results. I think my results where accurate because of my methods. I used a good reliable method that helps ensure that the test was fair in every way. ...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.

    oxidise and so might prevent the amount of hydrogen given off and it might affect the speed at which the magnesium and acid react. * Coil the magnesium ribbon every time so that it is all covered by acid. * Keep the same amount of magnesium and acid otherwise the

  2. Rates of reactivity.

    W1 Average weight finish (g) W2 Weight loss (g) W1- W2 0 20.30 20.30 0 1 20.30 19.8 0.50 2 19.8 18.95 0.85 3 18.95 17.75 1.20 4 17.75 16.12 1.63 5 16.12 14.32 1.80 6 14.32 12.47 1.85 7 12.47 10.56 1.91 8 10.56 8.58 1.98 9 8.58 6.38 2.2 10 6.38 4.18 2.2 Powder - Calcium carbonate (CaCO3)

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

    � Temperature of the acid If the starting temperature of the acid is different each time the speed at which the acid particles collide with the magnesium ribbon will increase more the higher the temperature goes. This means the acid particles move with more energy, which means they will collide

  2. 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

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

    I could use these results to calculate the initial rate of reaction. The weight before and after the experiment I could put the conical flask with the chosen volume of hydrochloric acid onto a set of accurate electronic scales and record the weight of it.

  2. Investigating the affect of concentration on the rate of reaction between magnesium and hydrochloric ...

    frequent so there is more chance of collisions with energy greater than or equal to the activation energy. Collisions are only effective if they have energy equal to or greater than the activation energy. The activation energy is the minimum amount of energy needed for a reaction to occur.

  1. What factors affect the rate of reaction between magnesium ribbon and hydrochloric acid?

    The variables that could be used are: 1. Concentration 2. Particle size/surface area 3. Pressure (for reactions involving gas) 4. Temperature 5. Light 6. Presence of a catalyst. These variables can be used because: 1. The more concentrated the reactants, the greater the rate of reaction will be.

  2. Find out the effect of concentration of acid, in thereaction between dilute hydrochloric caid ...

    We considered the factors in the reaction, and decided how we were going to control them.We kept our eyes on the experiment so that we could see exactly when we sholud�ve started the stop clock and stopped the clock. This way the rate of reaction(the time taken for the magnesium to disappear)

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