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# Rate of reaction

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Introduction

Rate of reaction In my piece of coursework I am going to investigate how concentration changes the rate of reaction. The chemicals I am going to be using will be magnesium and hydrochloric acid. The point of the experiment is to find out whether dilute or concentrated acid will react better with the magnesium. The formula and word equation for this is: Magnesium + hydrochloric acid = magnesium chloride + hydrogen. Mg+ 2HCl = MgCl2 + H2 Background knowledge The rate of reaction can be affected by four main factors which include temperature, concentration, surface area and catalysts. 1 Temperature- When gases or liquids are heated the particles gain kinetic energy and move faster. The increased speed increases the chance of a collision occurring between reactant molecules and the rate of reaction increases, before there are any chemical changes. The molecules have to have a collision and at minimum kinetic energy to fuse or react. 2 Concentration- Increasing the concentration also increases the probability of a collision between reactant particles because there are more of them in the same volume. ...read more.

Middle

Increasing the heat, meant the particles would be moving more vigorously, and would start to crash and break. An increasing in the surface area meant that there is more of a chance to have a reaction. My prediction The time taken for the magnesium will decrease as the concentration of the hydrochloric acid is increased. The more concentrated the acid is will increase the chance of collisions increasing. I have made this prediction from the information I collected about the collision theory. Variables I this experiment, I am going to be altering the concentration of the hydrochloric acid by diluting it with water. I will use a stopwatch to measure the time taken for the magnesium to react with the hydrochloric acid. To make this a fair experiment I will keep the length of magnesium the same length (1cm), the volume of acid and water at 50mls throughout and I will keep the temperature the same throughout as well (room temperature). Acid (cm) ...read more.

Conclusion

* The graph differs from 102's at 25/25 to 22s at 50/0. * As the concentration increases on the rate graph the rate increases. This agrees with my prediction. If the concentration is at 25/25 and it took 25s for the reaction to occur and then you double the concentration to 50/0 so it would take half the time because there are more particles colliding with each other. The time graph has a smooth curve this is shown on the graph following this page. The rate however has a straight line. Evaluation First I collected all of my equipment which was given to me by my teacher; I then collected information from the task and was therefore able to write a report on the project. I corrected myself and wrote out a sheet to guide me, step by step, through the experiment. After completing the experiment, I wrote out a final sheet of results and drew out two scatter graphs and rechecked my results to make sure everything was in order and all made sense. When the experiment was completed, I looked over the results and the experiment was a success. ...read more.

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