Investigating how the concentration of acid can affect the rate of reaction
Background
Magnesium + Hydrochloric acid ---> Magnesium chloride + Hydrogen
Mg(s) + 2Hcl (aq) --> Mgcl2 (aq) + H2 (g)
I intend to measure the rate of reaction by collecting the hydrogen gas produced and measuring the rate it is produced at.
I am aware that hydrogen is produced when acid “particles” collide with magnesium atoms to produce hydrogen molecules.
The variables which can affect the rate of hydrogen production are:
- The state of the magnesium, for example whether its ribbon or a powder.
- The volume of the acid.
- The concentration of the acid.
- Temperature.
- The container that reaction is carried out in.
The variable I will measure is rate calculated by measuring the volume of gas collected in a certain time.
How do Variables affect collisions?
- I think that if the magnesium is in powder form then the surface area is greater so there are likely to be more collisions between acid particles and magnesium atoms giving a higher rate of hydrogen gas production.
- If the volume of acid is increased then there may be more acid particles available to collide with the magnesium giving a higher hydrogen gas rate.
- If the concentration of acid is increased then this should as above give a higher rate.
- If the temperature is increased then the acid particles could absorb heat energy faster and hit the magnesium atoms more frequently and harder giving a higher rate.
- The shape and size of the container could change the depth of the acid in contact with the magnesium an affect collisions – increasing or decreasing chances.
