Coursework
Rates of Reaction
PLAN
Introduction
AIM - The aim of this experiment is to investigate the factor(s) affecting the rate of reaction when magnesium is reacted with dilute hydrochloric acid.
Background knowledge
This reaction takes place when particles collide with sufficient energy.
Variables - There are 6 main variables that you can change to increase the rate of reaction:
• TEMPERATURE - increasing temperature gives the particles more energy making them faster and will travel over a great distance in a given time and can collide easier overcoming activation energy.
• CONCENTRATION - increasing concentration means more particles in a given area making them easier to collide.
• STIRRING - stirring will make the particles move around more and help them collide with each other easier.
• CATALYST - catalyst is a substance, which increases the rate of reaction but itself remains the same.
Catalyst reduces the activation energy making the reaction quicker.
• SURFACE AREA - increasing the surface are by breaking up a particle into smaller particles so more of them will be exposed to successful collision.
• PRESSURE - increasing pressure increases the rate of reaction as you are pushing the particles together making there be more chance of collision.
MAGNESIUM + HYDROCHLORIC MAGNESIUM + HYDROGEN
ACID CHLORIDE
Mg(s) + HCl(aq) MgCl2(aq) + H2(g)
Prediction
I predict in this experiment that the increase in concentration of hydrochloric acid will increase the rate of reaction. This is because if there is an increase in the concentration their will be an increase in the amount of particles in a confined space which leads to an increase in the rate of reaction. When the number of particles increases there are more chances of the particles to collide with one another and reacting.
Apparatus
The rate of reaction will be measured in the gas syringe in cm/s.
Apparatus:
• 4 Magnesium strips of equal length
• 50cm dilute Hydrochloric acid
• Conical flask
• Gas syringe
• Measuring cylinder
• Stop watch
Rates of Reaction
PLAN
Introduction
AIM - The aim of this experiment is to investigate the factor(s) affecting the rate of reaction when magnesium is reacted with dilute hydrochloric acid.
Background knowledge
This reaction takes place when particles collide with sufficient energy.
Variables - There are 6 main variables that you can change to increase the rate of reaction:
• TEMPERATURE - increasing temperature gives the particles more energy making them faster and will travel over a great distance in a given time and can collide easier overcoming activation energy.
• CONCENTRATION - increasing concentration means more particles in a given area making them easier to collide.
• STIRRING - stirring will make the particles move around more and help them collide with each other easier.
• CATALYST - catalyst is a substance, which increases the rate of reaction but itself remains the same.
Catalyst reduces the activation energy making the reaction quicker.
• SURFACE AREA - increasing the surface are by breaking up a particle into smaller particles so more of them will be exposed to successful collision.
• PRESSURE - increasing pressure increases the rate of reaction as you are pushing the particles together making there be more chance of collision.
MAGNESIUM + HYDROCHLORIC MAGNESIUM + HYDROGEN
ACID CHLORIDE
Mg(s) + HCl(aq) MgCl2(aq) + H2(g)
Prediction
I predict in this experiment that the increase in concentration of hydrochloric acid will increase the rate of reaction. This is because if there is an increase in the concentration their will be an increase in the amount of particles in a confined space which leads to an increase in the rate of reaction. When the number of particles increases there are more chances of the particles to collide with one another and reacting.
Apparatus
The rate of reaction will be measured in the gas syringe in cm/s.
Apparatus:
• 4 Magnesium strips of equal length
• 50cm dilute Hydrochloric acid
• Conical flask
• Gas syringe
• Measuring cylinder
• Stop watch
