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

    pair on a water molecule and is eventually placed on the middle oxygen. Now one of the products of the reaction, ethanol is removed from the ion. With the charge spread across the carbon a proton is removed from the ion and placed on a water molecule, restoring the hydroxonium ion, and producing ethanoic acid.

  2. Antacid Investigation.

    so it shall equal = 1.6 cm cubed to neutralise the antacid. For Sodium Bicarbonate. Number of moles = 64 mg (0.064g) divided by 84 (RFM) = 0.00076 moles Number of moles of acid=1 x 0.00076 moles = 0.00076 moles of acid This number will be one because the reaction

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

    not included in the equation that I will use to work out the average. I created a second spinach extract solution using 20 grams of Spinach Oleracea. This was done so that I could compare my results from the two solutions and thus be able to detect whether one of the solutions had been contaminated.

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

    Altogether I tested 5 different concentrations of hydrochloric acid. 0.5M, which was the lowest concentration of acid that I used, there was only a tiny amount of gas evolved, but the time taken for the magnesium to completely react was over 700 seconds. 2.5M hydrochloric acid, which was the highest concentration that I used, produced the fasted rate of reaction.

  1. Investigating the Effects of Increasing Copper Sulphate Solution Concentrations on the Germination of Cress ...

    This occurs through enzymes (amylase, maltase, peptidases, lipase) changing the substances. The starch is broken down to maltose, which in turn is broken to glucose and transported as sucrose for cellulose or used for energy. The proteins in the seed are converted to polypeptides and then broken to amino acids, which are used for structural or enzyme proteins.

  2. Aspirin Investigation

    will be 70% for both reactions: Oil of Wintergreen --> Salicylic Acid, and Salicylic Acid --> Acetylsalicylic Acid. The calculations are based on my end product being 6g of acetylsalicylic acid (Aspirin). I am therefore assuming the overall yield to be 49% Working backwards: Aspirin 6g: moles = mass /

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

    Volume of water (ml) Time (s) 25ml 0ml 115.36 20ml 5ml 125.52 15ml 10ml 168.47 10ml 15ml 287.03 5ml 20ml 1374.69 Concentration of acid = Volume of acid *2 = x moles Total volume of solution 1) Concentration of acid = 25 *2 = 2 moles 25 2)

  2. Reactivity Series Investigation

    powder we are going to test for 2 minutes and so every powder will have 12 readings because there is 12 10 seconds in 2 minutes.So we are going to do calcium poder first and then magnesium powder and then iron filings and then zinc powder and then Aluminium powder.We

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