The Rate of Reaction Of Metals with Acids :: GCSE Chemistry Coursework Investigation

The Rate of Reaction Of Metals with AcidsIntroductionIn this investigating I will be looking at the send of receptionbetween a metal, which will be milligram ribbon, and an acid. Theacids will either be hydrochloric, ethanoic, sulphuric or phosphoricacid. I will be finding out if the activation energy changes dependingon whether a strong or weak acid is used. I will also be look intowhether or non there is a change in the instal of answer if a dibasicacid is used instead of a monobasic acid.PlanningThis investigation is therefore split up into separate experiments.Experiment 1 is to find the activation energy for the reactionsbetween hydrochloric acid and magnesium ribbon, then ethanoic acid andmagnesium ribbon. The only way to find the activation energy is totime how yen it takes for the reaction to complete at differenttemperatures. Experiment 2 is to find the order of reaction betweenmagnesium ribbon and hydrochloric acid, then sulphuric acid. There are some(prenominal) m ethods that can be used to find the order of reaction I could use an excess of magnesium ribbon and note down how much gas has evolved every 10 seconds until the reaction has finished. I could repeat the identical procedure as above, but with an excess of acid instead of magnesium ribbon. I could use an excess of acid and change the concentration, this would not require the reaction to be completed so I would have to time how long it takes for a set amount of hydrogen gas to form.There are several chemical equations that are relevant to thisinvestigation-Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g)Mg(s) + H2SO4(aq) MgSO4 + H2(g)Mg(s) + 2CH3CO2H(aq) Mg(CH3CO2)2(aq) + H2(g)3Mg(s) + 2H3PO4(aq) Mg3(PO4)2(aq) + 3H2(g)In my experiments I will not be using phosphoric acid due to timerestrictions and it is not relevant to the problems I am discussing,because it is a tribasic acid and I am comparing monobasic and dibasicacids.The equation needed to find the activation energy in a reaction isc alled the Arrhenius equation.In k = constant EA/R (1/T)Where k = rate constantEA = activation energy (J mol)R = gas constant, 8.31 J K molT = temperature in KelvinInitial Problems- The time restriction makes it extremely hard to find the order of reaction by timing how long it takes for all the magnesium to disappear.- I do not want to directly heat acid as this is dangerous when only