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

The aim of this investigation is to investigate the rate of reaction of magnesium (mg) with Hydrochloric acid (HCl). After studying the availability of equipment I have chosen to investigate how the temperature can affect the rate of reaction.

Extracts from this document...


AIM The aim of this investigation is to investigate the rate of reaction of magnesium (mg) with Hydrochloric acid (HCl). After studying the availability of equipment I have chosen to investigate how the temperature can affect the rate of reaction. Within this coursework, I am going to investigate how the concentration of hydrochloric acid effects the rate of reaction with magnesium, i.e. how quickly/how much hydrogen is produced. Aims Magnesium and dilute hydrochloric acid react together according to the equation below: magnesium + hydrochloric acid ??magnesium chloride + hydrogen The hydrogen produced makes the reaction mixture effervesce (fizz). The faster the reaction, the shorter the time taken for the effervescence to stop. You will study the effect of changing the concentration of hydrochloric acid on the rate of reaction. Hypothesis I predict that as the temperature increases, the speed of the reaction will increase therefore the gas will be produced faster. I believe this because most chemical reactions happen faster when the temperature is higher. At higher temperatures molecules mover around faster, which makes it easier for them to react together. Usually, a rise of 10OC will double the rate of reaction. ...read more.


After that I will measure 6ml of hydrochloric acid and 4ml of water and pour into another test tube and then place in the test tube rack. Finally I will measure 5ml of hydrochloric acid and then 5ml of water and pour it into the last clean test tube, and then place in the test tube rack. By using the stop clock, collect one strip of magnesium and drop it in the first test tube. As soon as the strip touches the acid start the stop clock. Observe what happens to the strip and note down any observations you can see. As soon as the strip is invisible stop the stop clock, and note down the time. I will do the same with the four concentrations. 8. To make the experiment a fair test repeat two times. Collect observations/results. Plan I am intending to react a 10cm length of magnesium ribbon with a chosen volume of hydrochloric acid. I will measure the rate of reaction by collecting the hydrogen gas that is produced in a gas syringe that will be connected, via a piece of rubber tubing and a rubber bung to the conical flask that the reaction will take place. ...read more.


10cm 6ml 4ml Exothermic, slow fizz 1:09 5. 10cm 5ml 5ml Slow fizz 1:16 How long the magnesium takes to dissolve Seeing as though I have chosen to measure the length of time it takes for the magnesium to dissolve - the only problem is with recording my experiment this way is that I could only settle on the average rate of reaction and not the initial rate of reaction. Therefore I will be using the initial rate to analyse the rate of reaction as it can calculate the true rate and not the average rate of reaction. Factors The factors that could affect the rate of reaction of my experiment are as follows: Concentration of acid This could affect the rate of reaction because the higher the concentration of the acid then the more acid particles per 100cm3 so more collisions per second and then there will be more successful collisions per second. � 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 with the magnesium with more energy, which will give more successful collisions per second. ?? ?? ?? ?? ...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

Here's what a teacher thought of this essay

This is a confusing and unstructured report. The basic elements are there but it lacks the structure to bring it together properly. There are specific strengths and improvements suggested throughout.

Marked by teacher Cornelia Bruce 17/04/2013

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

    Marble Chips and Hydrochloric Acid.

    4 star(s)

    The graph gives us a good device to prove that if you double the concentration the rate of reaction doubles. If you increase the number of particles in the solution it is more likely that they will collide more often.

  2. Peer reviewed

    An Experiment to Find the Amount of Heat Energy Released When 1g of Candle ...

    3 star(s)

    way, we can be more biased towards it when it is challenged by a different set of results. However, experiment 4 which suggests that there 21.911kJ of energy for every gram of candle wax was carried out in the exact same manner.

  1. A reaction between Hydrochloric Acid and Magnesium ribbon.

    Increasing the concentration of the reactants and raising the temperature bring about more collisions and therefore more successful collisions, increasing the rate of reaction. When a catalyst undergoes collision with the reactant molecules, less energy is required for the chemical change to take place, and therefore more collisions have sufficient energy for reaction to occur.

  2. The effect of temperature on the rate of reaction between magnesium ribbon and hydrochloric ...

    Dependent Variable (Variable that I am measuring): The time taken for all the magnesium ribbon to react with the hydrochloric acid is to be found with a stopwatch and rounded off to the nearest second. I will then find the rate of the reaction by dividing the time taken for

  1. The effects of caffeine on reaction time

    The pituitary gland sees all of the activity and as some sort of emergency occuring so it causes the adrenal glands to produce adrenaline. Adrenaline causes the breathing rate to increase, breaks down glycogen to glucose in the liver to provide energy for the metabolic processes, blood flow to the stomach slows and muscles tighten up ready for action.

  2. Experiment to Investigate the Rate of Reaction between Hydrochloric Acid and Sodium Thiosulphate, with ...

    not completely fair and it contained many experimental errors, most of which cannot be avoided, such as the change in the room temperature and if someone accidentally knocked the table on which the experiment was situated. I also predicted that the rate of reaction would decrease if the reaction progresses for long enough.

  1. To investigate the effect of the concentration of nitric acid on the rate of ...

    length of time, and record how much gas has been produced from the reaction at certain time intervals. VARIABLES AND COLLISION THEORY: There are four main factors or variables which influence the rate of a reaction, and they are: 1. TEMPERATURE 2. CONCENTRATION (or pressure for gases) 3. CATALYST 4.

  2. To investigate the effect of ph on the activity of trypsin.

    The juice that the pancreas secretes is alkaline so the ph that works best should also be alkaline. The temperature won't affect the reaction as I am going to keep it as the same temperature throughout the experiment. This is what I think will happen as the ph increases the

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