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

An Investigation to find out If Increasing the temperature of an acid Increases the reaction speed of Magnesium

Extracts from this document...


An Investigation to find out If Increasing the temperature of an acid Increases the reaction speed of Magnesium Introduction: A rate of reaction is measuring how fast two substances can react to form two new substances in a set period of time. The measurement of the reaction can take place by finding out how much of a new substance is formed. In most cases, and as in my experiment, the volume of gas produced can be recorded and in other experiments, the mass of a solid or the volume of a liquid can be found. When a reaction takes place, it is because bonds are broken and new ones are formed. In my investigation I am reacting hydrochloric acid (HCL) with magnesium (Mg). This will form magnesium chloride and hydrogen. Below you can see the formula for both, the reaction between hydrochloric acid and magnesium and the balanced symbol equation: This means that the hydrogen bond with chlorine is displaced by magnesium, therefore forming magnesium chloride. This proves that magnesium is higher in the reactivity series than hydrogen. Knowing that the reaction takes place through the displacement of bonds between magnesium and hydrogen, I can prove one other vital point. That is, that the hydrochloric and magnesium atoms must come in contact for the reaction to take place. Therefore, the rate of reaction can speed up or slow down depending on how many times hydrochloric acid particles and magnesium atoms collide. ...read more.


* Magnesium ribbons: 0.1g of magnesium ribbon for each test. Readings and Measurements: From the experiment I am going to take six readings. Each reading will be at a different temperature starting from 30�C going up to 80�C. At each range point I will take five readings which will be in minutes going up to five minutes of the overall time of each test. I will repeat the experiment twice so that I have two different sets of results. From these two sets I will get an average for each result. I have chosen to go up to 80�C because from my research I found out that after 80�C, hydrochloric acid starts to evaporate. This means that if I take my readings further on I will loose some acid because of evaporation. If I do lose any acid before the experiment, one of my variables, which is the volume of hydrochloric acid, will change and therefore lead to an unfair test. What I will be measuring in the experiment is the hydrochloric acid which I is going to be heated up, the magnesium ribbons and the hydrogen gas which is given off from the tests. The measurement units that I am going to use are: * ml: I will use millilitres to measure the hydrochloric acid from a measuring cylinder into a beaker and also to measure how much hydrogen gas I collect in the measuring cylinder from each test. ...read more.


So if you increased the temperature you therefore, are increasing the heat energy supplied to the atoms. This in turn increases the kinetic energy and the atoms move faster. If the atoms are moving faster they collide more often with each other and therefore, increase the rate at which they react. This means that I have one conclusion on the investigating the effects of temperature on the rate of reaction between hydrochloric acid and magnesium. That conclusion is: Evaluation: Looking at my result I can say that they are sufficient enough to draw up the conclusion which I have made and that they do not seem to bring out any extremely anomalous results. I have also noticed that the volume of the acid decreases as it is heated. This maybe due to the fact that hydrogen from the liquid evaporates from the solution. This may have thrown off the accuracy of the investigation. However, the chance that hydrogen evaporated is not as likely, as water. Because the hydrochloric acid has been diluted and there is a significant amount of water, making HCl less concentrated. However, at higher temperatures the water might have evaporated, and caused the concentration of the acid to increase. On the other hand I still think I carried out my experiment as carefully as I could making sure that all the test I took were fair. This is probably why my results look satisfactory and do not bring out any extremely anomalous results. From this I made out a good conclusion stating the difference that the temperature of an acid makes to a reaction. - 1 - ...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. Investigating the Effects of Increasing Copper Sulphate Solution Concentrations on the Germination of Cress ...

    planned, and some things which I had planned which should have been done better and there are a few things which I would change if I was going to do the investigation over again. Although I had planned to repeat each copper sulphate concentration 24 times, due to limitations I could not do this.

  2. See how different concentrations of Hydrochloric acid change the rate of reaction with a ...

    To work out the average I must firstly add up the three different times Concentration of Hydrochloric Acid (M) 1st Volume (ml�) 2nd Volume(ml�) 3rd Volume (ml�) Total Volume (ml�) 0.5 1 1 1.5 3.5 1.0 3.4 5 3 11.4 1.5 7 8 8 23 2.0 9.5 9 10 28.5

  1. Neutralisation Investigation

    We can also calculate the number of moles of acid being neutralised using this formula: V � C 1000 C stands for concentration (M), and V stands for volume (cm3). Volume of acid (cm3) Concentration (M) Moles (M) 20 2.0 0.04 20 1.6 0.032 20 1.2 0.024 20 0.8 0.016

  2. Rates of Reaction

    The tests will be repeated using the different concentrations of hydrochloric acid and different surface areas of the calcium carbonate. The calcium carbonate will be measured to the accuracy of 0.1g. The hydrochloric acid will be measured to the accuracy of 0.5g.

  1. Antacid Investigation.

    Number of moles in each chemical in Boots antacid tablet: For Calcium carbonate. Number of moles = 522 mg (0.522g) divided by 100 (RFM) = 0.00522 moles Number of moles of acid = 2 x 0.00522 moles = 0.01044 moles of acid Predicted volume of acid needed to neutralise the

  2. Aspirin Investigation

    It is also possible to use ethanoyl chloride or ethanoic acid. However using ethanoyl chloride results in the production of dangerous fumes of hydrochloric acid. The use of ethanoic acid results in a lengthy acylation procedure. Synthesis of Aspirin from Oil of Wintergreen The steps for the reaction route I

  1. How much Iron (II) in 100 grams of Spinach Oleracea?

    Place the conical flask containing the hot solution on a white tile. 17) Titrate the Potassium Manganate (VII) (aq) into the hot spinach extract solution until a pink colour appears. 18) Continue to add the Potassium Manganate (VII) (aq)

  2. The aim of this experiment is to answer the following question: What is the ...

    The colour will be deemed changed when I can no longer shake away the pink colour. This will indicate there are excess hydroxyl ions present in the solution. These ions are present in the Sodium Hydroxide solution and when they come into contact with the hydrogen ions in the sample solution they perform this reaction: H+(aq)+ OH- (aq)

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