To conduct this experiment I can use marble chips (calcium carbonate) or magnesium ribbon and in place of sulphuric acid dilute hydrochloric acid will be used. This is because sulphuric acid produces an insoluble salt which prevents any further reaction with the acid. The two possible equations for the experiment are: 1) Mg + 2HCl ”> MgCl + H 2) CaCO? + 2HCl ”> CaCl + CO + H O I have decided to conduct my experiment using magnesium ribbon and so equation 1 will be used. Here is a list of the factors which I could investigate: Volume of acid Concentration of acid.
Temperature of reaction Mass/length of magnesium ribbon Particle size (no. of strips of magnesium) The factor which I have decided to investigate is the volume of hydrochloric acid. The range of volumes I have opted to use are 10cmi?? , 20cmi?? , 30cmi?? , 40cmi?? and 50cmi??. The concentration of acid will remain at 2M throughout the investigation and the investigation will be conducted at room temperature. Also 1 strip of magnesium ribbon of mass 0. 05g will be used throughout the investigation.
For each volume of acid used I will time how long it takes for 50cmi??of hydrogen gas to be produced and collected in a gas syringe. Apparatus Conical Flask (with bung) 100cmi?? gas syringe Scales Measuring cylinder Stopwatch Hypothesis I believe that as the volume of acid increases so will the rate of gas produced. This is because there will be more acid molecules and so there will be more chance of collisions between the magnesium and hydrochloric acid, thus a higher rate of reaction. I believe that the volume of acid will be directly proportional to the rate of reaction and so the following will be true:
Therefore, if the volume of acid is doubled then the rate of gas produced should double. Diagram Method First of all the gas syringe was connected to the conical flask. 0. 05g of magnesium ribbon was weighed using the scales and placed inside the conical flask. The first volume of 2M hydrochloric acid, 10cmi?? , was measured out using a measuring cylinder and then added to the flask. Simultaneously the stopwatch was started and the bung was placed on the conical flask. When 50cmi?? hydrogen had been collected the stopwatch was stopped.
This was repeated 3 times with each of the volumes of hydrochloric acid, 10, 20, 30, 40 and 50cmi??. For each volume an average time was calculated and then using that time the rate of reaction was calculated with the following equation: Rate (cmi?? /s) = Volume of gas produced (cmi?? ) Time (s) Results Time Taken (s) Volume of HCl (cmi?? ) Reading 1 Reading 2 Reading 3 Average Reading Rate of Reaction (cmi?? /s).