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

Investigate what affects the speed of reaction between Hydrochloric Acid (HCl) and Magnesium Metal (Mg).

Extracts from this document...

Introduction

Science Investigation - Reaction Rates Planning the Investigation TASK - You are to investigate what affects the speed of reaction between Hydrochloric Acid (HCl) and Magnesium Metal (Mg). For a chemical reaction to take place, certain that must occur. First of all, the reacting particles, atoms, molecules, or ions, must collide. For them to be able to collide, there must also be enough energy in the collision to break the chemical bonds in the reacting molecules. If the particles do not have enough energy to break the bonds, the particles will just bounce off one another. A collision that has enough energy to result in a chemical reaction is referred to as an effective collision. This is called the collision theory. What happens when Magnesium and Hydrochloric Acid react? Magnesium + Hydrochloric Acid Magnesium Chloride + Hydrogen Mg (s) + 2HCl (aq) MgCl (aq) + H (g) With these chemicals, there are several things that you could measure. You could measure the amount of gas given off in a certain amount of time or how long it takes for the reaction to stop. I was going to investigate the amount of gas produced at different temperatures. ...read more.

Middle

* Timer. * Sand paper. * Lab coat. * Goggles. DRAWING OF APPARTUS Step-By-Step Plan Due to my preliminary work, I notice that 20cm� of gas (hydrogen) was given off. Therefore, I will have a better understanding of when the reaction will finish. Anything in bold type are areas where safety is needed. (1) Clear area, make sure stools and bags are under tables. (2) Set up apparatus. (3) Put on goggles. (4) Heat Hydrochloric Acid (HCl) to specific temperature. (5) Take beaker off heat. (6) Swirl HCl. This is to try and get an even temperature throughout the beaker and make the experiment fairer. (7) Add magnesium ribbon to solution. (8) Quickly attach cork to prevent any gas being let out. (9) Start stopwatch as soon as possible. (10) When reaction is finished stop the stopwatch and record the time. (11) Repeat the experiment. (12) After the experiment is finished, clear apparatus. I will repeat this experiment three times and make an average afterwards. The more times you repeat an experiment the more accurate it will be at the end. Due to the amount of time, I will only be able to repeat the experiment three times. ...read more.

Conclusion

Nevertheless, for me to say 'start timer' and my partner to actually start the timer, gas is still lost. Again a similar problem occurs when stopping the timer. It is hard to tell, when the reaction has fully stopped. During the experiment, I had to estimate when the reaction had finished. Magnesium reacts with the oxygen in the air, just like iron reacts with water and turns into rust. This layer on the magnesium will make the test unfair if it is not removed. So, we used sand paper to remove it. The problem with this is that when you sand down the Magnesium strip, you are also removing Magnesium. Therefore, the amount of Magnesium is not the same with each strip. If this experiment was done on a bigger scale, I think it would affect the reaction greatly. However, as this is not, I do not believe that sanding the Magnesium had a significant affect on the experiment. If I were to do this experiment again, I would measure how much gas is given off every 10 seconds. For me to be able to do this, I would have to use a lower concentration of HCl because the reaction is very rapid. I would also repeat the experiment, to get a more accurate average. ...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

    The Effect of Concentration on the Rate of Reaction between Magnesium [Mg] and Hydrochloric ...

    4 star(s)

    If you reduce the size of particles itself then it increases the rate of reaction as it also increases the surface area available for collisions to occur. This then has an effect on the number of collisions there are as it increases, however it does not affect the energy used.

  2. Marked by a teacher

    The aim of this investigation is to investigate the rate of reaction of magnesium ...

    According to my research on the Internet if temperature is increased the rate of reaction also increases - this is due to the chemical particles receiving kinetic energy. If more kinetic energy is present in the particles, the particles move faster, this also means the particles will be colliding with each other often.

  1. Rates of Reaction - HCl + Mg

    Catalyst: A catalyst gives the reactants a surface to stick to where they can collide with each other. This definitely increases the amount of collisions. Also, catalysts increase the rate of reaction by helping break chemical bonds in reactant metals and provide a 'different pathway' for the reaction.

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

    This heat energy will then be converted into kinetic energy and the atoms will collide more often. So if you increase the temperature you increase the amount of kinetic energy and therefore, increase the rate of reaction. The collision theory comes into play concerning the speed.

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

    And the rate of reactions increases. 3. Rate increases with surface area. An Increase in the surface area of reactant exposes more atoms for reaction i.e. there is a greater chance of successful collisions. For example, the collision of acid (hcl)

  2. Rates of reaction between Magnesium and HCl.

    to produce hydrogen gas as shown. When the magnesium ribbon reacts with the hydrochloric acid, magnesium chloride is formed. Mg(s) + 2HCl (aq) MgCl2 (aq) + H2 (g) Magnesium+hydrochloric acid magnesium chloride +hydrogen The hydrogen gas produced will be collected by the displacement of water. The reaction between magnesium and hydrochloric acid is exothermic.

  1. Find out how different concentrations of HCl affect the rate of the reaction with ...

    ACID + BASE -------> SALT + WATER. They also react with metals to give salt and hydrogen gas. ACID + METAL -------> SALT + HYDROGEN. What acids have in common is that they produce hydrogen ions when they dissolve in water. Acids are also proton donors and lone pair acceptors.

  2. Investigate the reaction between Magnesium (Mg) and Hydrochloric Acid (HCl)

    Once this has been done I will insert into the solution a 1cm strip of magnesium (Mg), when the magnesium touches the solution I will immediately start timing by using the stopwatch. As soon as the magnesium has visibly disappeared I will stop timing and record the time in seconds by using a table.

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