How the concentration of Hydrochloric Acid effects a reaction with magnesium Introduction: In this experiment I will be looking at how the concentration of acid affects reaction rates, this all relates to the collision theory which states: "When particles of one substance have enough energy to collide with the particles of another substance, we say that a reaction is taking place. When the particles finish colliding the reaction is over." Many factors can affect the rate of reactions, they are: Temperature: when increased the particles move faster, which means these particles take a part in more collisions.
Concentration: If the solution has a higher concentration it means there are more particles within the same volume, so more collisions occur.
Surface Area: If one of the substances are broken up you increase the surface area. So that the solution has a larger area to react with, this increases the rate of reaction.
Catalysts: A substance that increases the rate of reaction without being used at all its self.
This experiment can be related to another experiment which uses marble chips and hydrochloric acid. The results are taken from how long it takes to collect a certain volume of Co2.
Diagram Students investigated the effect of increasing the acid concentration and the relationship to the rate of reaction. The experiment was repeated twice at 1.0 molar, 1.5 molar and 2 molar.
Adapted From "Complete Co-ordinated Science "" Chemistry" List of apparatus required 3 Beakers 30 Cm of Magnesium Ribbon (In Total) Glass Rod Measuring Cylinder Goggles Stop Clock 750ml of Hydrochloric acid (In Total) Prediction I think that the higher the concentration the faster the reaction will occur. Because the higher the concentration the more molecules there are to react with the magnesium ribbon.
The molecules collide with the magnesium...