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

To investigate the effect of concentration on the rate of a reaction - Magnesium + Hydrochloric Acid ---> Magnesium Chloride + Hydrogen.

Extracts from this document...

Introduction

To investigate the effect of concentration on the rate of a reaction Magnesium + Hydrochloric Acid ---> Magnesium Chloride + Hydrogen Mg(s) + 2HCl(l) ---> MgCl2(l) + H2(g) Aim The aim of this investigation is to find out how the concentration of Hydrochloric Acid effects the rate of the reaction. In this case we will measure the rate at which Hydrogen is produced. The concentration of the Hydrochloric Acid will be our variable. Prediction I believe that the higher the concentration, the faster the rate of reaction. From preliminary experiments I have discovered that the higher the concentration of the acid, the more collisions there are. Therefore, the rate of reaction will be larger if we use a high concentration of the acid rather than using a smaller concentration. Procedure Experiment Acid Volume (cm3) Water Volume (cm3) Total Volume (cm3) Concentration (mol/dm3) 1 50 0 50 1m 2 40 10 50 0.8m 3 30 20 50 0.6m 4 20 30 50 0.4m 5 10 40 50 0.2m For the experiment we have chosen specific equipment. The equipment we have chosen was used in our preliminary experiment as was the magnesium. ...read more.

Middle

Reading 1 Reading 2 Reading 3 Average of Readings 0 0 0 0 20 3 2 2.5 40 4 3 3.5 60 4 4 4 80 4 4 4 100 5 4 4.5 120 6 6 6 Key Variables There are 4 main variables that will effect our experiment, these variables are: * Volume * Concentration * Surface Area * Temperature These variables are kept under control in our experiment. * Volume is kept at a constant of 50cm�. * Concentration will vary. See table on first page (it will go from 1m to 0.2m). * Surface area of the Magnesium is kept constant by making sure that we prepare the magnesium the same for each experiment (coiling it up) and we will use magnesium ribbon only. * Temperature will be kept roughly the same(room temperature). To improve our experiment we could use a water bath to keep temperature the same. The same amount of heat will be produced in this experiment as our preliminary experiment but there is much less effect as we have used 30cm3 more of the solution. Hotter the atoms, the more they vibrate, they more they collide, this could therefore effect the rate on certain experiments if the temperature is not kept constant. ...read more.

Conclusion

* Sources of error in the procedure could have been due to: 1. Varying length of magnesium (human error) 2. The concentrations were slightly off due to bad measurements with the pipette. 3. The balance is accurate to 0.01g so it is unlikely that this will have caused any noticeable errors. * The sources of error are due to apparatus used and human error. Using more accurate equipment (scales which measure the magnesium to a greater accuracy) and taking more care when preparing the experiment could reduce these anomalies. * By altering our method and using more accurate methods of cutting up the magnesium, and rolling up the magnesium carefully so that the surface area exposed is the same we could have more reliable results. * The data is very trustworthy due to the fact that we took two readings. The likely hood of error decreases as we take more readings. The average of the readings that matched closest was taken to ensure that our results were even more precise. * Our preliminary experiment data and graph also backs up our results. * My prediction "I believe that the higher the concentration, the faster the rate of reaction" was correct and has proven successful. To investigate the effect of concentration on the rate of a reaction Jonathan Middleton, 11B Page 1 5/2/2007 ...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

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

    The Effect of Concentration on the Rate of Reaction between Magnesium [Mg] and Hydrochloric ...

    4 star(s)

    We will be timing how long a solid takes to dissolve in a solution; it may use the same time intervals as the other 3 strategies. We will be timing it until however long it takes for the solid to completely disappear within the solution so there are no traces of solid left after the stop watch is stopped.

  2. Marked by a teacher

    Investigation of the rate of reaction between Magnesium and Hydrochloric acid

    4 star(s)

    0 0 0 0 0 0 30 15 37 45 32 32 13 60 30 46 52 50 49 6 90 39 49 56 56 54 7 120 43 51 59 57 56 8 150 45 52 61 59 57 9 180 46 53 62 60 58 9 210 46

  1. Marked by a teacher

    The aim of this investigation is to investigate the rate of reaction of magnesium ...

    The procedure for the experiment is as follows; * Using a measuring cylinder, measure 10cm3 of water and pour it into the side arm tube. * Measure 10cm3 of hydrochloric acid (1 mol/ dm3) and add it to the water.

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

    Repeat steps 1-8 for the five different concentrations of nitric acid (2 molar, 1.6 molar, 1.2 molar, 0.8 molar and 0.4 molar). (See conversion table) N.B.: At least people should be involved in conducting the experiment to make the process a little easier resulting in better, more accurate and more reliable results (which is what I did).

  1. Determine the rate equation for the reaction of hydrochloric acid with magnesium metal, and ...

    From this graph the activation energy is 18kJ mol-1, to two significant figures. Sources of error The method I used to determine the activation energy of the reaction between hydrochloric acid and magnesium is very simple, and has few sources of error.

  2. Finding the effect of concentration on the rate of reaction of magnesium ribbon with ...

    Therefore there is a greater chance in a more concentrated solution of acid particles colliding, and reacting, with particles on the surface of the magnesium. As to give an example of an increase in rate of reaction in modern life.

  1. Investigating the Rate of Reaction Between Hydrochloric Acid (Hcl) and Magnesium (Mg).

    If you add more heat energy (i.e. increasing the temperature) then the atoms will have more kinetic energy and therefore move faster. If they are moving faster the rate of reaction increases because the atoms will collide more often and more and the reaction will speed up.

  2. Rate of reaction of hydrochloric acid and mangesium ribbon.

    The factors that may affect the rate of reaction are:- temperature of the Hydrochloric Acid, mass of the magnesium ribbon used, concentration of the Hydrochloric acid, surface area of the magnesium ribbon used All of these factors will change the rate of reaction because of the Collision Theory.

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