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

Scientific Investigation: How Temperature Affects The Rate Of Reaction Between Magnesium And Hydrochloric Acid!

Extracts from this document...

Introduction

Scientific Investigation: How Temperature Affects The Rate Of Reaction Between Magnesium And Hydrochloric Acid! Planning I'm planning on investigating how temperature effects the reaction between magnesium and hydrochloric acid, the experiment will show whether the reaction will speed up or slow down with the change in temperature. Temperatures will range from room temp up until 70 degrees. The investigation will be a fair test because all quantities will remain the same for each test, each test will use the same amounts of hydrochloric acid and same size of magnesium, also the concentration of the acid will also not be changed. APPERATUS; * Conical flask * Bunsen Burner * Thermometer * Tri-pod * Protective matt * Stopwatch * Gauze * Measuring jug * Goggles Whilst doing the experiment there are many things that will have to remain the same in order to keep the tests fair, these include amounts and measurements as well as concentration and size and shape of the magnesium e.g. ...read more.

Middle

feel that the test will show me that as the temperature increases the time for the reaction to completely take place will decrease. I came to my prediction through seeing in past tests and experiments throughout the year that temperature has increased many rates of reaction, so I believe the same will occur in this test. Data The results I obtain will be stored in a table; the results will be recorded on both temperature and time enabling me to give a clear graph showing my results. I will record the rate at which the magnesium reacts in hydrochloric acid at temperatures of; room temp (27), 40, 50, 60, 70 degrees, at each temperature, magnesium will be added to the acid, and the rate at which it takes to fully react and disappear will be recorded. Method 1. Collect all equipment. Tests In Seconds Temperature (degrees) Test1 Test2 Test3 Average Room Temp (27) 68 70 73 70 40 62 60 64 62 50 60 65 59 61 60 50 51 49 50 70 47 ...read more.

Conclusion

60degrees could of actually been over and at 63degrees. Other factors affected the investigation; these factors are minor things such as delays in timing response and slight different sizes of magnesium. Many things, not massive factors, but very minor factors give slightly non accurate answers. These inaccuracies are unavoidable and are due to human abilities, factors couldn't have been made any more accurate unless done by machine. Evaluation I am pleased with the investigation results and the way, in which the tests were taken, even though the tests worked well they still were not completely accurate. All results matched my prediction and all results point towards my prediction. My results support my conclusion, as the temperature of hydrochloric acid increases the rate at which the magnesium react decreases. The results show clearly this conclusion and also once again back up my prediction. To improve my investigation I would carry out the test double the amount of times and at more frequent temperatures, I would also use a water bath to keep the temperature of the acid the same throughout the reaction. ...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 Aqueous Chemistry 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 Aqueous Chemistry essays

  1. Free essay

    Chemistry investigation

    * Clamp- This is attached to the retort stand. * 50 ml measuring cylinder- To measuring the hydrochloric acid accurately * stop-clock- To measure the time of the reaction * 10ml of Hydrochloric Acid plus varying amounts of water- To measure the concentration of the acid * Magnesium ribbon (3cm per experiment)

  2. Indigestion Tablets Investigation

    From this point on I used 2 delivery tubes carefully put together and sealed at the joint. This provided ample length for the rest of my experiments and from that point on I did not have any problems with the length of the delivery tube.

  1. Antacid Investigation.

    + 2 HCl (aq) --> Ca Cl2 (aq) + CO2 (g) + H2O (l) Magnesium carbonate (s) + Hydrochloric acid (aq) --> Magnesium Chloride (aq) + Carbon Dioxide (g) + Water (l) Mg CO3(s) + 2 HCl (aq) --> Mg Cl2 (aq) + CO2 (g) + H2O (l)

  2. Aspirin Investigation

    The compound, called salicin, is found in the white willow tree. Around 200 B.C., Hippocrates, the Greek physician known as the father of medicine, discovered that chewing on willow bark could relieve pain and fever. Although ASA was a proven pain reliever, no one really knew how it worked until more than 70 years after Hoffmann's discovery.

  1. Reactivity Series Investigation

    will happen like calcium reacting with oxygen and this is very dangerous so no powders will be in the flame.Wearing gloves prevents the powders to get on your skin which may Corrosive. Symptoms of redness, pain, and severe burn can occur.Don't inhale the calcium or Inhalation produces damaging effects on the mucous membranes and upper respiratory tract.

  2. I am investigating the rate of reaction between magnesium and hydrochloric acid.

    concentration - Effects of surface area - Effects of a catalyst - Effects of stirring Safe Test Before I carry out this experiment I must make sure it is safe.The main points of safety are: - Wear safety goggles at ALL times.

  1. Rates of Reaction Investigation

    The rest is water. About 20 percent of all sulphuric acid is now made by the lead-chamber process, but that percentage is diminishing. The second method of manufacturing sulphuric acid, the contact process, which came into commercial use about 1900, depends on oxidation of sulphur dioxide to sulphur trioxide, SO3, under the accelerating influence of a catalyst.

  2. What effects the rate of a reaction

    Other reactions are very slow, e.g. the rusting of iron. For practical reasons, reactions used in the laboratory for studying rates of reaction must not be too fast or too slow. Collision theory The particles of reacting substances collide with each other and a fixed amount of energy called the activation energy (Ea)

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