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

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Chemistry Coursework: Rates of Reaction

Name: Mohammed Tahmid Azad

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

By Mohammed Thamid Azad

Candidate Number- 5021

Centre Number- 13317

Rates of Reaction

INTRODUCTION – This coursework will be investigating the effect of concentration on the rate of reaction between a metal-Magnesium [Mg] and Hydrochloric Acid [HCL]. Rate of reaction is the measurement of how quickly a reaction is progressing. It also includes how much products are being formed and what portion is being used up. Rate of reaction just means ‘the speed of the reaction’. It is measured by the rate of formation of a product. When you are doing an experiment in order to make a product you should know how long the reaction takes to complete, before the product is produced. This coursework will be experimenting the reaction speed of Magnesium Metal with Hydrochloric acid. I will be observing ‘the rate of reaction between Magnesium and Hydrochloric acid to measure how long a solution takes to react within different level of concentrations. ‘In the experiments it is predicted that the reactions are not at a steady rate, meaning that they begin at a curtain speed then decrease until they stop which then decreases the concentration of reactants.

AIM- To investigate the effect of concentration of acid on rate of reaction

Mg(s) +2HCl (aq)  MgCl2(aq) +H2(g)

HYPOTHESIS/PREDICTION

I predict that if there is more concentration within a solution then it means there are more particles of reactant moving around water molecules which increase the chance of collisions between the particles happening.  Therefore I my hypothesis is that the more concentration there is within a given space then the more chance there Is of a successful collision increasing the rate of reaction.

THEORY

Rate Equation:

Average rate= change in the volume of hydrogen/ time for the change to happen

Factors that affect rate:

Collision Theory (KE) - Collision theory was introduces by  and  in 1916. Chemists believe that the theory explains how the various factors affect reaction rates. It is believed that molecules are only able to react if they bump into each other. When molecules are colliding with each other it can lead to other theory’s affecting this such as concentration, temperature and catalysts. The theory states that when molecules are colliding with one another atoms can break and new bonds form creating new molecules. There are molecules in gases and liquids which are always in constant motion colliding in millions. Many reactions are not successful only some are successful and this is because some reactions have collisions in which the molecules are moving around giving the bonds the strength to break (activation energy). If you increase the concentration of the reactions and the temperature it brings more collision and therefore the success rate is higher increasing the rate of reaction. If there is a catalyst present the collision between the molecules, requires less energy for the chemical change to take place, therefore more collisions have enough energy for the reaction to occur, which in term increase the reaction rate.

Concentration-

          (2Mol)                             (4Mol)                              (6Mol)

   6 PARTICLES               12 PARTICLES               18 PARTICLES

  • Higher Concentration so more particles in given space.
  • More chance of successful collision (overcome activation energy)
  • Increased rate of reaction

The more concentration there is within a dissolved reactant, the quicker the rate of a reaction. The higher the concentration the more particles present within a given space this then result in a higher chance that the particles colliding with each other and therefore increasing the rate of reaction.

The different concentrations within a given space varies, this means that the more particles there are the more likely they are able to collide with one and another and this increases the chance of collisions forming products.

For example there are fewer particles present in 0.5mol concentration compared to a 2mol concentration, therefore in a less concentrated solution of acid the number of collisions is lower as there are less acid particles to collide with one another. 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. Rate of reaction increases due to more particles being present with a given space. “The increased concentration within the reactants has a higher rate of recurrence of collisions between the magnesium and Hydrochloric acid”

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When the collisions are taking place we need to make sure if they successful so that it is reaching the activation rate breaking the bonds allowing the rate of reaction to increase.

Surface Area-

        (2cm)                          (1cm)

       

        2x2=4                              1x1=1

        4x6=24cm2               ...

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This is a well written and structured report with an appropriate range of data. Small improvements have been suggested throughout.