Investigation Rates of Reaction Investigation
Aim: To investigate the effect of concentration on the rate of reaction between hydrochloric acid, water and magnesium. I am investigating the following reaction: Mg + 2HCl MgCl2 + H2 Magnesium + Hydrochloric Acid Magnesium Chloride + Water During this investigation we will be trying to find out how much affect different concentrations of hydrochloric acid has on the production of hydrogen (product) over a total volume of 100 cm 3 within sixty seconds. Our teacher had already organised for us to work in pairs of two and our partner throughout the investigation. Our teacher had also given us a rate of reaction pack, where I found the following equation on the first page (page 238). Mg (s) + 2HCl (aq) MgCl2 (aq) + H2(g) Rate of reaction=Amount of reactant used or product formed / Time I also found the following formulae in our provided rates of reaction pack:
Average rate=Change in the volume of hydrogen / Time for the change to happen.
Variables which may affect the rate of reaction:
1) Temperature (potentially a little temperature rise could double the rate of reaction - particles can only react when they collide. If you heat a substance the particles move faster and therefore collide more frequently. This will speed up the rate of reaction) 2) Existence of catalyst (chemicals that speed up chemical reactions therefore the rate - Only a minute quantities of the catalyst is needed to produce dramatic change in the rate of reaction) 3) Surface area of solids (bigger surface area contributes to speeding up a reaction - you are only going to get a reaction if the particles in the gas or liquid collide with the particles of the solid. Increasing the surface area of the solid increases the chances of...