• 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

    Rate of Reaction Chemistry Coursework

    4 star(s)

    So for this investigation we performed a preliminary investigation so we could understand the sort of equipment that we should be using and the sort of chemicals that we should be reacting and the amount we should be using. So after looking at the task that has been set I

  2. 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.

  1. 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.

  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. A reaction between Hydrochloric Acid and Magnesium ribbon.

    For a reaction to occur the reactant particles must collide. Only a certain fraction of the total collisions cause chemical change; these are called successful collisions. The successful collisions have sufficient energy (activation energy) at the moment of impact to break the existing bonds and form new bonds, resulting in the products of the reaction.

  2. To investigate the effect of concentration on the rate of a reaction - Magnesium ...

    Reading 1 Reading 2 Reading 3 Average of Readings 0 0 0 0 20 23 24 23.5 40 48 48 48 60 69 70 69.5 80 83 84 83.5 100 98 97 97.5 120 x x X Concentration: 0.6mole 30cm3 HCl : 20cm3 H2O Time (seconds)

  1. Investigate the affect of temperature of sodium thiosulfate and hydrochloric acid against rates of ...

    * I must measure the temperature of the thiosulfate solution at the same point in each experiment - before I add the acid. * I must use the same cross, as one cross could have a darker shade that another.

  2. The effects of caffeine on reaction time

    Caffeine effects part of the nervous system that controls respiration so that more oxygen is pumped through the lungs. Caffeine also causes the brain blood vessels to constrict because it blocks adenosine ability to dilate them. This causes you to have an increased neuron firing in the brain.

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