We learned that if the concentration doubles, the rate doubles. I will therefore choose the dilute sodium Thiosulphate to prove this and to see if it affects the rate of the reaction. Besides concentration I know that catalysts, temperature and surface area also affect the rate of the reaction. Therefore I think that the less concentration of sodium Thiosulphate the slower the rate of the reaction will go. We did preliminary work on this experiment, I took a conical flask and put 50cm³ of sodium Thiosulphate and added 10cm³ of Hcl.
I will use this to measure out the Hydrochloric acid and Distilled water because there volume together will equal 10cmÂ³. If I use a 50cmÂ³ Measuring cylinder, I won't be able to get a good enough accuracy. Stopwatch- For timing the experiment Pipette for measuring out accurately and piping back excess Hydrochloric acid Piece of paper with a black cross on it like this: To find out when the experiment has ended. It is dark and thick because I want to clearly see when the experiment has finished Paper towels: For washing beakers and measuring cylinders out. [IMAGE] 1.
As I already know that increasing one quantity will speed up the reaction as the particles are more likely to collide. In this investigation several measures will need to be done to make sure that the results I get will be precise. From the planed method I can work out what will need to be done to achieve the best results possible. I will also need to think about what other factors may vary my results to someone else’s and how this could be improved. Equipment Needed: · Beaker · Test-tube · Piece of paper with a cross on · 25ml² of Sodium Phiosulphate · 5ml² of Hydrochloric Acid Factors about the equipment that may affect the results: The amount of one particular quantity, or concentration of the acid.
Planning Aim --- The aim of my experiment is to investigate if the speed at which the limestones are dissolved is changed by how concentrated the acid is. Equipment To do my experiment, I will need beakers, a paper spoon, a stop clock, limestone powders, stirring rod, measuring cylinders and an electronic balance for powders Plan For this experiment, I will use 30mls of the acid each time and 1gm of powdered calcium carbonate. The concentration of the acid will be changed by adding water and less acid each time. First, I will use a paper spoon to spoon out the limestone powder and weigh it on the electronic balance. Next, take out the excess powder until the weight is 1gm.
I will then put the powdered marbled chips in the chronicle flask along with the acid and put the stopper on top. I will then record how long it takes for it to fill the measuring cylinder up. I will repeat each experiment 4 times so I can work out an average Prediction: I predict that when I have a higher concentration I will have a faster rate of reaction. I believe this is so because as you increase the concentration of the acid, there are more acid particles in the same volume. Therefore there is a greater chance of acid particles colliding, and reacting with more particles on the surface of the marble.
I will be reacting magnesium with sulphuric acid to test if the concentration of an acid affects the reaction time. I will use molars between 0M & 1M for my initial trial run. I will measure the rate of reaction using a conical cylinder with a rubber bung & a gas syringe. I will then time how long it takes to fill up to 100cc of gas. I will repeat each concentration 3 times then take a average so I get more accurate results, I will repeat any anomaly's I get so I will get my final results as accurate as possible.
Method I will weigh out one gram of marble chips using a balance and put it in a conical flask and add to it a concentration of 50cm3 using water and hydrochloric acid. I shall start by filling up a measuring cylinder with water and putting it in a water bath so I can record how much gas has been given off. I shall then put my one gram of marble chips measured using in a conical flask then add to that my concentration of hydrochloric acid and water, put on the bung and start the stop clock. I shall record how long it takes for 25cm3 of gas to be collected. The reason I chose to do this investigation was because I have
Next, the hydrochloric acid will be added to the Na2SO3 (thiosulphate). At this point, the stopwatch will be started, and then the time recorded for the cross to disappear. This will then be done with the concentration of Na2SO3 increasing in measurements of 10ml each time. I will change the ratio of water and hydrochloric acid such as 50:0, 40:10, 30:20, 20:30, 10:40, 0:50. This will allow me to determine what ratio is needed for the reaction to occur quickest (i.e.
There are several methods 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 same 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 this investigation:- 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 time restrictions and it is not relevant to the problems I am discussing, because it is a tribasic acid and I am comparing monobasic and dibasic acids. The equation needed to find the activation energy in a reaction is called the Arrhenius equation.
Since our initial reading of the burette was 0.62 mL with a pH of 2.31, a subtraction of our initial reading from each of our burette readings is needed in order to obtain more accurate readings. The titration was continued until a jump occurred between the pH indicating that an equivalence point had been reached somewhere between the jump. Next a more accurate titration was performed, meaning recording more data points around the equivalence point by adding smaller amounts of base. The pH meter was calibrated again, and 50 mL of Formic Acid was dispensed into a 250 mL beaker. The pH meter was placed in ... ... middle of paper ... ... data due to students not finishing their titration in time.