Chem
CHEMISTRY
INVESTIGATION
‘HOW DOES CONCENTRATION AFFECT THE RATE OF REACTION?’
SANIA HUSSAIN
CANDIDATE NUMBER:5093
Contents
The aim – PG 1
Introduction – PG 1
Theories – PG 1, 2
Prediction – PG 2, 3
Safety – PG 3
Strategy – PG 3, 4
Method – PG 5, 6, 7
Preliminary – PG 7
Actual experiment and graphs – PG 7+
Chemistry coursework Hypothesis/Aims The aim of the investigation is to see how different concentrations of hydrochloric acid affects the rate at which hydrogen gas is produced when it’s reacted with a strip of magnesium. The rate of reaction is a measure of change that happens in a single unit of time. When a reaction takes place the particles of the reactants collide. The more often the particles collide the more likely they are to react and so the faster the reaction is. The speed at which a reaction takes place can vary and depend on a number of factors:
The surface area of any solid reactants
The concentration of reactants (including pressure in the cases of gases)
The temperature
The presence of a catalyst
In this particular investigation hydrochloric acid and magnesium will be reacted to produce hydrogen, and therefore one of the main factors will be the concentration of the reactants. In order for magnesium and acid particles to react together:
They must collide with each other
The collisions must have enough energy
The independent variable in this particular reaction is the concentration of the hydrochloric acid. Each time the concentration will be increased by 0.25 moles. This will ensure that our readings are close and help when working out the rate of reaction. So that it will be easier to make comparisons. The dependent variable will be the volume of hydrogen gas produced and this will be measured using the inverted measuring cylinder. The constant variables, which are to be kept the same, include: the temperature, the length & thickness of Mg, the volume of diluted acid, the
INVESTIGATION
‘HOW DOES CONCENTRATION AFFECT THE RATE OF REACTION?’
SANIA HUSSAIN
CANDIDATE NUMBER:5093
Contents
The aim – PG 1
Introduction – PG 1
Theories – PG 1, 2
Prediction – PG 2, 3
Safety – PG 3
Strategy – PG 3, 4
Method – PG 5, 6, 7
Preliminary – PG 7
Actual experiment and graphs – PG 7+
Chemistry coursework Hypothesis/Aims The aim of the investigation is to see how different concentrations of hydrochloric acid affects the rate at which hydrogen gas is produced when it’s reacted with a strip of magnesium. The rate of reaction is a measure of change that happens in a single unit of time. When a reaction takes place the particles of the reactants collide. The more often the particles collide the more likely they are to react and so the faster the reaction is. The speed at which a reaction takes place can vary and depend on a number of factors:
The surface area of any solid reactants
The concentration of reactants (including pressure in the cases of gases)
The temperature
The presence of a catalyst
In this particular investigation hydrochloric acid and magnesium will be reacted to produce hydrogen, and therefore one of the main factors will be the concentration of the reactants. In order for magnesium and acid particles to react together:
They must collide with each other
The collisions must have enough energy
The independent variable in this particular reaction is the concentration of the hydrochloric acid. Each time the concentration will be increased by 0.25 moles. This will ensure that our readings are close and help when working out the rate of reaction. So that it will be easier to make comparisons. The dependent variable will be the volume of hydrogen gas produced and this will be measured using the inverted measuring cylinder. The constant variables, which are to be kept the same, include: the temperature, the length & thickness of Mg, the volume of diluted acid, the