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

Investigating varying concentrations, affecting the Rate of Reaction between hydrochloric acid (HCL) and magnesium (Mg)

Extracts from this document...


GCSE Chemistry Coursework Investigating varying concentrations, affecting the Rate of Reaction between hydrochloric acid (HCL) and magnesium (Mg) Candidate name: Alexander Willink Aim: The aim of this experiment is to find out the effect of concentration of acid, in the reaction between dilute hydrochloric acid and magnesium ribbon. Prediction: I predict that with an increase in concentration the rate of reaction will there for also increase. This will (I predict) be proven by the amount of hydrogen gas produced. If we increase the concentration, we are in essence, increasing the total number of collisions. This, in turn, will increase the number of effective collisions, and the rate will increase. Introduction: magnesium + hydrochloric acid magnesium chloride + hydrogen Mg (s) + 2Hcl (aq) MgCl2 (aq) + H2 (aq) For a successful collision reaction to take place the reacting particles must collide with enough energy, this energy will need to be sufficient to break the magnesium bonds. Room temperature should be adequate. The rate of reaction can be measured by how many successful collisions occur in units of time, (the amount of hydrogen gas produced). When the concentration increases, so will the reaction. This is because there should be more particles to react with the magnesium. Whilst magnesium and hydrochloric acid particles are making successful collisions their particles are forming magnesium chloride and hydrogen. ...read more.


when the Concentration of HCL increases. The theory states that if, the more concentrated the Reactants, the greater the number of collisions between particles increases. This also explains why the greatest rate of reaction is usually as soon as the reactants have been mixed, i.e. they are both at their highest concentrations. As the reaction continues, the Concentration of the reacting substance decreases and so does the rate of reaction. We must consider what happens when a reaction takes place. First of all the particles of the Reacting substances must collide with each other, and secondly a fixed amount of energy Called activation energy* (Ea) must be reached for the double bonds to be broken into single ones. If the Particles can produce the right amount of energy (i.e. if they collide fast enough and in the Right direction) a reaction will take place. The reaction is speeded up if the numbers of Collisions are increased. In this investigation we must consider the topic of variables. Clearly, the time taken for the magnesium to disappear when it is placed in different concentrations of HCL is related in some way. The higher the concentration of HCL you use, the less time it takes for the magnesium to disappear and so the rate reaction increases. The concentration of HCL you use is the independent variable because it will Vary, and the time taken for the rate of reaction to take place (i.e. ...read more.


I submitted all the results to a computer program called excel, where, by using a formula, I was easily able to subtract each starting value from each set of results. By doing this, it would create the illusion that all experiments started at 0cm�. 7. I should have been more accurate in cutting the magnesium; my graphs prove that the magnesium was cut inaccurately. I would expect all the results to end at the same level. This, however, is not the case. One other explanation of the inaccuracy (you must understand I am trying to shift the blame a little) is the constant minor change in room temperature, emphasized by the fact that the tests were not executed all in the same setting. 8. I could also have gained more results by simultaneously recording the temperature. I could then ensure that the reaction was taken whilst in similar temperature conditions....different temperatures. How is done. 9. Another anomaly that is clearly spotted in the graph is the different concluding results for each experiment. I expected all the results to level out at roughly the same level. However there is a clear difference between 10. The line of best fit drawn from the graph can see the accuracy of the results. If it is clear that a point is not following the line, then it can be accounted for as an anomaly. There may be many reasons for such an occurrence. 1 1 GCSE Chemistry Coursework Alexander willink Chemistry coursework 2003 Page 1 of 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 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)

    So within the solution there is less a chance of an acid particle hitting a magnesium particle making the rate of reaction slower. However within a higher concentration of acid such as 2mol the number of acid particles is greater, therefore increasing the chance of an acid particle hitting a magnesium particle.

  2. Marked by a teacher

    For my experiment I am finding out the effects on the reaction rate when ...

    3 star(s)

    I used distilled water instead of tap water because there is almost no chance of impurities mixing with distilled water so you can be sure that there are no different ions unlike tap water (which gives it a good taste).

  1. Rates of reaction between Magnesium and HCl.

    In this particular investigation using a catalyst was not applicable. The surface area could be used, however this was fairly difficult to do, and the results would see fairly inaccurate, due to the time and equipment that we were provided with.

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

    The collision theory comes into play concerning the speed. When the atoms gain more kinetic energy they move around faster, and therefore more atoms collide more often. * Concentration of the acid If you increase the concentration of the acid you increase the number of hydrochloric acid particles in the solution.

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

    The temperature of the reaction mixture rose by 7.5�C during the reaction. Because increasing temperature raises the rate of reaction, this affected my results. The increase in temperature could be reduced by having the boiling tube containing the reaction mixture in a water bath maintained at room temperature.

  2. Factors Affecting Enzyme Activity

    Below is the method I would use if I were to investigate the affects of temperature on enzyme activity. Method for temperature investigation From my own scientific knowledge I know that catalase is commonly found in human livers and that human body temperature is approximately 37.5�C therefore I predict that

  1. Find out how the rate of hydrolysis of an organic halogen compound depends on ...

    Rate = ?[reactants] (where ? refers to the change) ?t The initial rate will be taken, therefore the gradient line will start at zero, and thus Y1 and X1 will equal 0. From this it can be shown that, Rate = Y2 - 0 X2 - 0 = Y2 X2 Therefore, for concentration 0.2 cm3: rate = 196 /

  2. An Investigation into the factors affecting the rate of reaction between magnesium and hydrochloric ...

    A 100cm3 gas syringe should be appropriately accurate for measuring the gas produced since it is accurate to 1cm3 of gas. I will use a three figure balance to measure the mass of magnesium to be used since it is vital that as close to 0.1g of magnesium is used as possible.

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