The aim of my experiment is to find out the rate of reaction between Hydrochloric acid (HCL) and Magnesium (Mg) in different temperatures. The products that will be formed are Magnesium Chloride (MgCl2) and Hydrogen (H2).
I predict that as the temperature increases the rate of reaction also increases. To further explore the fact I further predict that the rate of reaction will double for every 10ÃÂ° C rise in temperature. I further predict as the temperature rises by 10ÃÂ° C the rate of collisions will also double. Thus if the collisions double then the reaction between Magnesium ribbon and Hydrochloric acid will also more or less double.
The particles of any gas or liquid can only react if they are supplied with energy. Thus at low temperatures the particles just bounce of each other since they do not have enough energy. The reaction happens only when the particles gain kinetic energy and thus move faster.
This increased speed increases the chances of the collisions between the reacting molecules.
Before any change takes place on the collisions the molecules must reach a minimum kinetic energy called the Activation energy. The activation energy is the most important factor in terms of temperature and reaction speed. Thus if the temperature increases then more kinetic energy is obtained by the particles and so at a higher temperature there is a greater proportion of them have reached the desired activation energy to react. This means that there is a higher chance of collisions thus increasing the speed of reaction since most of the particles have enough energy to react.
Constants and variables:
-Amount of Hydrochloric acid (15 cm3)
-Concentration of Acid (0.6 Molars).
-Length of the magnesium ribbon ( 1 cm).
-The type of container being used.