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

An Investigation Into the Rate of Reaction Between Hydrochloric Acid and Magnesium- Planning

Extracts from this document...

Introduction

AN INVESTIGATION INTO THE RATE OF REACTION BETWEEN HYDROCHLORIC ACID AND MAGNESIUM - PLANNING The aim of this investigation is to find out the effect of the rate in the reaction between hydrochloric acid (HCl(aq)) and magnesium (Mg(s)). Before beginning the experiment of finding out the effect of the rate of reaction between hydrochloric acid and magnesium, I will have to understand the meaning of rate of reaction and the factors that affect it. Collision Theory The rate of a chemical reaction is a measure of how fast the reaction takes place. A chemical reaction only occurs when particles collide (hit each other). The collision theory describes how the rate of reaction increases (the amount of hydrogen produced per second) when the concentration of hydrochloric acid increases. ...read more.

Middle

The minimum energy which is required in order for the particles to collide is called the activation energy. It is important to remember that a rapid reaction is completed in a short period of time. Some reactions are very fast e.g. an explosive. There are factors that may affect the rate of reaction, which are as follows: * Temperature. * Mass of a reactant. * Concentration of acid. * Surface area of a reactant. * Type of acid. All of these factors will change the rate of reaction because of the Collision Theory. Investigation In this investigation I will test different concentrations of hydrochloric acid reacting with magnesium. In the reaction between hydrochloric acid and magnesium ribbon, the hydrochloric acid will dissolve the magnesium and produce hydrogen gas. ...read more.

Conclusion

Na (Sodium) Li (Lithium) All too dangerous to react with a strong acid. Ca (Calcium) ...... Mg (Magnesium) Al (Aluminium) Manageable metals. These metals will react with hydrochloric acid as they are higher in the reactivity series than hydrogen and so a displacement reaction will take place. Zn (Zinc) Fe (Iron) ...... H (Hydrogen) ...... Cu (Copper) Pb (Lead) None of these metals will react with hydrochloric acid as they are all lower in the reactivity series than hydrogen, therefore a displacement reaction will not happen. Ag (Silver) Al (Gold) Depending on certain factors the rate that this reaction will take place will either increase or decrease. Question? My question is to see that if I change the concentration of the Hydrochloric acid for each experiment I will see an increase or decrease in the rate of reaction between Hydrochloric acid and Magnesium ribbon. ...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. Determine the rate equation for the reaction of hydrochloric acid with magnesium metal, and ...

    I am using 0.005 moles of HCl, so the magnesium is 0.025/0.005 = 5 times in excess. This shows that at all times the magnesium is in a large excess. Observations When the magnesium was added to the hydrochloric acid in the boiling tube, the reaction mixture started to fizz:

  2. The aim of the investigation is to examine the kinetics involved in the reactions ...

    1.00M Ethanoic acid (weak acid) + magnesium ribbon: TEMP/o C TEMP/K (1/TEMP) in K-1 TIME /s Experiment 2 /s AVERAGE /s-1 RATE 1/av time /s-1 In (rate) 20 293.0 0.00341 520.33 512.33 516.33 1.9x10-3 -6.26 30 303.0 0.00330 330.22 327.81 329.02 3.0 x10-3 -5.81 40 313.0 0.00320 220.48 200.41 210.45

  1. Rates of reactivity.

    Rates of reaction increase in the presence of catalysts, substance that provide a new, faster reaction mechanism but the are unchanged or regenerated so that they can continue the process. Mixtures of hydrogen and oxygen gases at room temperature do not explode.

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

    The first is to find out what the initial rate of reaction would be for concentrations 1.25M hydrochloric acid and 1.75M hydrochloric acid as it would be interesting to see how the rate increases compared to 1M hydrochloric acid. Another experiment that I could do is change the type of acid that I use.

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

    However, this does not happen in my experiment and the rates of reaction increase as the temperature increases. However, something which I had predicted does not represent itself in my results. My prediction was, that even though the rate of reaction would increase the final volume of gas collected would be the same for all temperatures.

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

    Introduction In the reaction between hydrochloric acid and magnesium ribbon, the hydrochloric acid will dissolve the magnesium and produce hydrogen gas. All chemical reactions involve reactants which when mixed may cause a chemical reaction which will make products.

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