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

Displacement Reactions of Metals.

Extracts from this document...

Introduction

Louise King 25th March, 2002 Displacement Reactions of Metals Task Investigate the effect of having pieces of metal in contact with solutions of other metal salts. Required Apparatus 3 Copper Strips 3 Zinc Strips 1 small cup of Silver Nitrate 1 small cup of Copper Sulphate 1 small cup of Lead '2' Nitrate 6 small test tubes 1 test tube rack 3 small pipettes Safety For this experiment you have to wear a white lab jacket or apron, protective glasses and a pair of gloves. As we are dealing with potentially dangerous gases so precautions have to be taken. In this experiment it is essential to wear protective gloves as if any acid falls onto your hand it could cause permanent damage. ...read more.

Middle

with Silver Nitrate. Then repeat this with the other solutions; Copper Sulphate and Lead '2' Nitrate. A simplified version of this is shown below: Now leave the test tubes for between 20-40 minutes. By now on some of the strips, small crystals should have formed and this will be noted in our table of results. After the experiment is over we need to pour the contents of our test tubes into different beakers and not down the lab sinks. The last thing we need to do is to put all our equipment away. Results Below is a table showing my results. I have included the solution, metal and then a comment of what I saw: Solution / Metal Silver Nitrate Copper Sulphate Lead '2' Nitrate Copper Grey Crystals (of silver) ...read more.

Conclusion

However, when we mixed the copper strip with the Lead '2' Nitrate, no chemical reaction occurred. This is because the copper is not high enough in the activity series to replace the lead so no reaction takes place. When we dipped the zinc strip into the Copper Sulphate, the zinc displaces the copper. The previously blue copper solution looses its colour in the reaction and the zinc gets coated in a dark red-brown copper metal. To conclude: with a more reactive metal (one higher up in the activity series) will always displace a less reactive metal (one lower down in the activity series) from its compounds. The more reactive metal takes away the non-metal from the less reactive metal. Displacement reactions can be very useful in our daily lives as they are frequently used to produce electricity in batteries. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Physical Chemistry 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 AS and A Level Physical Chemistry essays

  1. Double Displacement Reactions

    Place this mass of the reagent into the flask which is marked with the reagent. 4. Measure out 5 ml of distilled water in the 10 ml graduated cylinder, and place this water in the flask with the reagent. 5. Stir the reagent so as to combine it completely.

  2. Investigating the Rate of the Reaction between Bromide and Bromate Ions in Acid Solution

    The value of Pearson's Product Moment Correlation Coefficient for these results is 0.981, again suggesting strong positive linear correlation. This leads me to the conclusion that the reaction is first order with respect to the concentration of bromate ions. CONCLUSION 2: (Equation 3.5.2)

  1. Investigating how concentration affects rate of reaction

    I was able to clearly prove the correct order of reaction for each of these chemicals by using my graphs of concentration against reaction rate. To work out the overall order of the reaction all of the individual orders of reaction must be added together.

  2. Electrochemistry - Inventing Better Batteries

    Background Electrochemistry is a branch of chemistry that studies chemical reactions which take place in a solution using two metals and two different electrolytes which are described as half cells. The metals used are also named electron conductors and the ionic conductors (the electrolyte)

  1. Alkaloids are the most diverse group of secondary metabolites and over 5000 compounds are ...

    This was sometimes successful as for example, the suggested pathway to the isoquinoline alkaloid is as follows: It is possible to divide the biosynthesis of the alkaloids into two categories according to whether products are obtained from the amino acids ornithine and lysine, or the aromatic amino acids phenylalanine, tyrosine, tryptophan.

  2. Types of Chemical Reactions Lab

    As molecules warm up they begin to vibrate more and the chances of them bumping in to one another increases - the more bumps that happen, the faster the reactions go. It is represented by the equation AB ? A + B or (in the case of the lab) CuSO4?5(H2O)(s)

  1. Activity Series of Metals Lab

    An exothermic reaction occurs when the energy need to break the bond in the reactant is less than the energy released upon the formation of products. In an exothermic reaction heat if release. However Endothermic is the complete opposite, the energy required to break bond in the reactant is greater than the energy released upon the formation of the product.

  2. Outline and examine some uses of different metals through history, including contemporary uses, as ...

    Faraday?s principle of electromagnetic induction led to the development of the dynamo, this meant that electricity could be produced in sufficient quantities for the use in Hall-Heroult processes involving the electrolysis of molten aluminia and cryolite to produce aluminium. The development of advanced machinery sped up chemical processes, allowed more

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