Rate of Reaction Investigation Plan In this experiment I will be investigating the rate of reaction and the time taken for a 1cm strip of magnesium to entirely disappear in a container of hydrochloric acid. The equation for this reaction is magnesium + hydrochloric acid or Mg(s) + 2HCL = MgCl2 (aq) + H2 (g) For experiment my input variable will be the concentration of Hydrochloric acid, so I will be using a concentration scale of 1-2 mol dm-3. My prediction is that the higher the concentration of hydrochloric acid the faster the rate of reaction will be. Below is a graph showing my predicted results: I am basing my prediction on the premises that when the solution of water and hydrochloric acid is dilute there are less hydrochloric acid molecules in the solution. Making it is less likely that they collide with the magnesium particles decreasing the speed of the reaction; therefore the more concentrated the solution is the more hydrochloric acid molecules there are and therefore there will be more reactions as these molecules or particles collide with the magnesium.
The other important independent variable that will affect the speed of the rate of reaction is the length of magnesium ribbon. We need to put enough Mg Ribbon into the HCL so that it doesn’t run out straight away but also so that the experiment stops by itself once the gas syringe has filled up. The reasons for choosing these two independent variables are that it would be too hard to try and find a catalyst for this experiment; a catalyst is a substance that increases the rate of a chemical reaction without being consumed in the reaction. Finding a catalyst for this particular experiment could take months never mind the amount of time we have been given for our experiment. The independent variable that I will change is going to be the hydrochloric acid, we will use 50ml of HCL at the following molarity concentrations; 2molar, 1.6molar, 1.2molar, 0.8 molar and 0.4 molar.
I will be measuring this by timing how long it takes for the magnesium to be no longer visible and there is no hydrogen released. Prediction: I think that when Hydrochloric acid of the same volume come in to contact with Magnesium of different lengths of ribbon,, the rate if reaction for the longer strip would be far slower than the shorter one. I believe that this as the collision theory tells us that molecules collide which cause to react and merge to create a compound. This reaction varies in speed depending on the amount of molecules in the mixture and how much energy the molecules possess, which is why heated molecules react faster than normal ones. So with the amount of Hydrochloric acid staying relatively the same yet the number of Magnesium molecules increasing, the reaction will only take longer as the molecules have to collide even more for the reaction to be complete.
In this experiment, the first two reactions are exothermic so the temperature of the solution and container will rise and some heat will be lost to the surroundings. Purpose: The purpose of this experiment is to calculate the heat of formation of magnesium oxide by studying a series of reactions involving magnesium and magnesium oxide and using Hess’s Law. Hypothesis: If the heat of reaction is found for two equations, then Hess’s Law will be able to determine the heat of reaction of the desired product. Materials: • S... ... middle of paper ... ...actual heat of reaction for Part II was -146kJ/mole. The heat of formation found for the formation of liquid water was -286kJ/mole.
This will happen because if the pH level of a liquid is lower, the hydrogen ions will consume the electrolytes, hydrogen ions are also being consumed and the element starts corroding faster. Trials: There were 3 trials for each level of pH level in liquids and a total of 9 trials throughout the experiment. Multiple trials are required to make sure the data corresponds to the research. It is important to have several trials to make sure the data being collected at the end of the experiment is parallel and is related to each other. More trials help the scientist conducting the experiment to have more accurate results and to see if a mishap or error occurred early in the experiment.
In the experiment the magnesium reacts with hydrochloric acid and it makes magnesium chloride and hydrogen gas. The can determine the mass of the starting magnesium, without actually weighing it. Purpose In the experiment, the purpose would be to find the mass of the magnesium without actually physically weighing it on the scale. Instead by seeing how much gas is produced from the hydrochloric acid reacting with the magnesium. Hypothesis Possible if the magnesium reacts with the hydrochloric acid then magnesium chloride and hydrogen gas would be produced and the mass of the original sample of the magnesium could be found because the gas that would be produced is going ...
Investigating Factors that Affect the Rate of Reaction Between a Metal and an Acid Factors that may affect the experiment + fair test The variables that could affect the rate of reaction are the temperature, amount of magnesium, concentration of acid, surface area of magnesium and volume of acid. The variable I am going to change is the concentration of acid. I am going to measure how long it takes a piece of magnesium(no more than 20m in length) to react in different concentrations of acid. When magnesium is placed into hydrochloric acid, it reacts by the acid particles colliding with the magnesium particles. I am doing the experiment, using the magnesium in ribbon form.
For example, a more detailed hypothesis could be that if I double the temperature, the rate of reaction will double as well (e.g. 20 c has a reaction time of 10 seconds whist 40 c has a reaction time of 5 seconds) Here are diagrams to demonstrate the kinetic and collision theory. Apparatus Magnesium ribbon 40cc sulphuric acid Beaker Measuring cylinder Thermometer Tripod Gauze Heat Mat Bunsen Burner Stopwatch Method To begin the experiment I will measure out 40cc of sulphuric acid into a measuring cylinder and then pour it into a beaker. I am not certain how much magnesium to use that will best react with 40cc of sulphuric acid. So before I start the final experiment I will carry out a preliminary test to discover whether a 2cm, 3cm, or 4cm accurately measured piece of magnesium ribbon is most efficient when doing the final experiment.
* You can also use the method of obscuring a cross with sodium thiosulphate and time which cross becomes invisible first. I am going to use a syringe to measure the amount of carbon dioxide given of at regular intervals. This is because it is accurate as the smallest division on it is 1ml. The important variables are: * Temperature – if it is increased the reaction as the particles will have more energy. * Number of calcium carbonate chips – if there are a lot of chips more carbon dioxide will be formed.
As soon as the acid reaches the correct temperature a 5cm strip of magnesium shall be placed in the acid and the bung put in the top of the tube. Simultaneously, a clock will be started to time how quickly the glass syringe fills. I will measure the amount of gas produced in equal time intervals such as 10, 20, 30 etc. ====================================================================== Scientific Explanation ---------------------- [IMAGE]For a chemical reaction to occur, reactant particles must collide. Successful collisions are when two particles hit head on.