Aim: To investigate how concentration affects the rate of a chemical reaction between Hydrochloric Acid and Magnesium.
Mg(s) + 2HCl (l)MgCl + HHypothesis: I think that the greater the concentration of hydrochloric acid, the faster the reaction will take place.
Explanation of Hypothesis: Most chemical reactions go faster when the concentrations of the reactants are increased. This is because in order for any reaction to happen, those particles must first collide. If the concentration is higher, the chances of collision are greater because more particles are present therefore the frequency of collision increases and this increases the speed of reaction. Which is why I think that the greater the concentration of Hydrochloric acid used, the faster the reaction will take place.
Apparatus:Measuring CylinderTest-tube Holder4 Test-tubesDropperStopwatchHydrochloric Acid (2M)Hydrochloric Acid (1M)WaterRulerMagnesium RibbonVariables:Independent Variable: the concentration of hydrochloric acid used.
Dependent Variable: the time taken for the magnesium ribbon to dissolve which will change when the concentration of the hydrochloric acid is used.
Constants:Length of magnesium ribbon used-1 inchVolume of reactant (hydrochloric acid) used-5 mlRoom temperature and pressureProcedure:1)Cut out 4 pieces of Magnesium ribbon, each 1 inch in length.
2)Mix 2.5 ml of 1M HCl with an equal volume of water to form 0.5M HCl.
3)Mix 2.5 ml of 1M HCl with an equal volume of 2M HCl to form 1.5M HCl.
4)Pour the 5 ml of 0.5M HCl into a test-tube and add a piece of magnesium ribbon.
5)Record the time taken for the entire ribbon to dissolve.
6)Repeat the procedure with the 1M, 1.5M and 2M HCl.
Observations:No. Concentration of HCl (M)Time Taken (s)Speed=1/time (s-1)10.531230.000322124720.0004131.511960.00084421940.0052I observed that when the magnesium ribbon was added to HCl, the temperature of the mixture immediately increased which led me to believe that it was an exothermic reaction. Besides this increase in temperature, I observed that...