Magnesium Strip Reaction

Rates of Reaction Investigation

The aim of this experiment is to investigate the effects of changing the concentration by the rate of reaction. By conducting this experiment, it helps us develop a method for measuring the volume of gas generated in a reaction between Magnesium and Hydrochloric acid. We can then distinguish a relationship between the mass of magnesium reacted and the volume of hydrogen generated.

I predict that increasing the concentration of hydrochloric acid will shorten the amount of time taken for the maximum amount of hydrogen to be collected, indicating that the rate of reaction has increased. This is because increasing the concentration ensures a higher level of particles in a solution, increasing the chances of collisions.

This is the effect of the collision theory, where there are a higher number of collisions in a system, more combinations of molecules will occur. The reaction will go faster, and the rate of that reaction will be higher.

Method:

- Set up apparatus as shown in the diagram below

- Add 50ml of hydrochloric acid into the beaker

- Measure 40 mm long strip of magnesium ribbon

- Add the 5cm of magnesium to the hydrochloric acid

- connect the long thin tube into a conical flask

- insert a rubber stopper for the tube to enter

- fill a container with water and place an upturned measuring cylinder filled with water into it

- start timing

- measure the amount of gas collected

Variables:

- Keep the same volume (independent)

- Keep the same length of magnesium (independent)

- Change the amount of acid (dependant)

- Change the amount of water (dependant)

- Temperature of reactants, amount of reactants & atmospheric pressure (controlled)

The rate of the reaction is to be measured by timing and recording with/along side the amount of Hydrogen dispersed.

Discussion

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