The original diagram shows how the solution will be with 1M hydrochloric acid and 5cm of magnesium strip. I think this because of the Collision theory. The effect of temperature on a reaction rate In this experiment I shall be investigating how temperature affects the rate of reaction Rates of reaction The Factors that affect the rate of reaction are temperature, surface area, concentration, catalysts, light and pressure Surface area — Surface area is the amount of solid surface that is available for reaction - Only affects solids so this will not affect our experiment - When the surface area increases the rate of reaction increases as there is more surface area for the particles to work on, thus, there are more collisions per second - Example : It is easier to light a fire with small pieces of stick than using large blocks of wood Concentration - Concentration is the amount of molecules of a substance in a given volume - Concentration affects solids, gases and liquid so this will affect our experiment - When the concentration increases. A piece of magnesium ribbon can be added to a solution of hydrochloric acid. I predict the higher the temperature, the faster the reaction rate. Next I had to attach the bung on the conical flask, and the rubber tubing that is attached to, it to the syringe.
Continue timing until no more gas appears to be given off. Choose only one indicator that signifies end of reaction. If the temperature is too high, the enzyme molecules vibrate too vigorously and the enzyme is denatured: it loses its 3D shape and will no longer bind with a substrate. In this experiment, the independent variable is the change in concentration of the sulphuric acid. At higher acid concentration, the rates of bubble forming were rapid than those in lower acid concentrations were.
It reacts with zinc to produce Zinc. The results for each 10 second interval were not accurate enough and there was not enough magnesium to get a high level of hydrogen. Retrieved March 8, 2012, from chemguide. Additionally ill try and be as accurate as possible while taking the readings of the thermometer and time it accurately so that I get the most accurate times. Prediction: I predict that the heating the hydrochloric acid will effect it as heating is one… 1541 Words 7 Pages Introduction In this chemical reaction, the magnesium will dissolve in the hydrochloric acid to produce hydrogen gas.
Collect 10mL of 2M hydrochloric acid using a 10 ml glass pipette. Aims and objectives of the experiment The aim of this experiment is to verify the effects of surface area of solid reactants and concentration of aqueous reactants on the rates of acid-base chemical reactions. Magnesium metal in form of a ribbon or powder reacts with acids rapidly than water liberating hydrogen gas. Here is what apparatus I will use: Draw Apparatus I will wear goggles due to the fact that I am handling acid. The reaction happens only when the particles gain kinetic energy and thus move faster. This is because of some slightly changing variables around the room and in the experiment even though I tried my best to keep the variables constant.
I will be performing the experiment by measuring out the time taken for the Hydrochloric acid and the Magnesium ribbon to react at different temperatures. Silver ions are reduced to silver. The particles of any gas or liquid can only react if they are supplied with energy. If you were to use cubed limestone it wouldn't be fair as no cube will be exactly the same size. I also needed safety goggles at all times to protect my eyes from the corrosive hydrochloric acid.
Most of these variables 479 Words 2 Pages Science Coursework — What factors effect the rate of reaction between magnesium and hydrochloric acid? This was probably by not putting on the bung fast enough when the magnesium was inserted into the acid. When the two chemicals react, a displacement reaction will take place and the magnesium will displace the hydrogen in the hydrochloric acid forming magnesium chloride and hydrogen gas. I tried this and the results were much more reliable to use and analyze. Given that, the experiment was carried out under the same conditions, the data obtained are reliable and generalizable. The temperature that the reaction is occurring at The temperature at which the reaction is taking place should be kept constant. The evolved hydrogen is collected in a water-filled measuring cylinder, and the amount indicated at 5-second intervals is recorded and it continues until the reaction finishes. Before any change takes place on the collisions the molecules must reach a minimum kinetic energy called the Activation energy.
Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. Use MathJax to format equations. Apparatus Pyrex Beaker Gauze Tripod Bunsen Burner Stopwatch Thermometer Measuring Cylinder Experimented Materials i. I predict that a reaction rate for a 2M solution will be double the rate for 1M because it's double the particles. In order to control this, the amount of hydrochloric acid must be recorded carefully and kept constant. Predesigned Data Table Concentration 3M 2.
This line graph clearly shows that as the temperature increases so does the speed of the reaction, shown by a reduction in the time taken. Magnesium Aluminum Zinc Iron Copper Prediction: Aluminum will be. There are many variables that I can change, which are the temperature and concentration of the hydrochloric acid, and the mass and the surface area of the magnesium strip. I will also clean my test tube after every test I carry out and dry it so that there is no water in there so that I can have the most accurate results. This is to compare with the other diagrams to see what the change is and if the reaction rate has decreased or increased. This should in theory increase the rate of reaction as the temperature is increased.
When I put in the 8cm of cleaned magnesium in with the acid, I started the stopwatch and put the rubber bung quickly over the flask to prevent gas escaping. This means that there will be a higher chance of the calcium carbonate molecules colliding with the hydrochloric acid and reacting, with enough energy to break the activation barrier. The balanced formula for this. © Nuffield Foundation and the Royal Society of Chemistry Page last updated October 2015 This is a resource from the Practical Chemistry project, developed by the Nuffield Foundation and the Royal Society of Chemistry. Safety goggles will be worn throughout the investigation as the reaction could fizz violently and cause eye damage if it was to spit.
The magnesium strips were cleaned and cut correctly by the lab technician and I measured and inspected the strip each time I started the experiment to make sure it was ok for the experiment. Cut magnesium ribbon by 1mm intervals and put them into each test tube which have different concentration. Safety goggles and gloves Avoid rubbing eyes or skin while handling the liquid. As I can see on the two graphs as the concentration increases the initial rate increases. To learn more, see our. The magnesium strips were cleaned and cut correctly by the lab technician and I measured and inspected the strip each time I started the experiment to make sure it was ok for the experiment.