In a chemical reaction more than two reactants are put together which makes a new product. For successful reactions to take place particles of different elements or compounds need to collide, and react together. A successful reaction happens when successful collisions take place. For successful collisions, particles must collide with enough energy to give a sufficient amount of force when colliding. From this you can see that in order for a reaction to take place, collisions between reacting particles need to happen.
Activation energy represents the minimum energy needed to break bonds with reactants, with this they can react forming a new product’s’. Two reactions colliding with enough energy new product The reaction that I will be investigating is the reaction between hydrochloric acid and magnesium ribbon. I will use different concentrations of hydrochloric acid to see the affects, outcomes and the time taken. As the reaction proceeds I will time how long it takes for the magnesium ribbon to fully dissolve, this happens because the magnesium reacts with the hydrochloric acid.
Magnesium + hydrochloric Acid ==>? Magnesium Chloride + H2O Mg(s) + 2Hcl(aq) ==>? MgCl + H2(g) I will decide when my reaction has stopped by observing the magnesium ribbon and when it is out of sight and there are no more bubbles I will stop the timer. There can be some problems with this method; there is a human eye observing it and deciding when to stop the timer and so that means it cannot be as accurate, also observing the bubbles will be hard because the bubbles are quite small.
Because this method isn’t very accurate a more reliable way to decide when the reaction has stopped is observing the syringe, as when the syringe stops moving it means there is no more hydrogen being produced which means there is no more products being produced there for the reaction has stopped. Key Factors: That could affect the rate of a chemical reaction… A reaction takes place when there are two or more reactants trying to neutralise each other to create a new product.
Reactions occur when particles of different elements or compounds collide and react together. The particles need a minimum amount of energy to make the reaction happen; this is called the activation energy. Listed below are the things that contribute in making the reaction happen quicker and slower. These key factors make successful collisions. There are factors that speed up the process of a reaction and slow them down. The key factors that will the rate of the chemical reaction are: Catalyst Concentration Surface area Temperature.
Increasing the temperature increases the rate of reaction, this is because when a reactant has been heated, more energy then required if given to the reactant making the particles move faster. This results in more frequent collisions causing a much faster rate of reaction. I will be using this factor in my experiment, however I will keep the temperature the same to ensure my test is fair. However this factor will affect my experiment because the room temperature cannot be kept constant at all times. Catalyst A catalyst is a substance that speeds up are chemical reaction without being chemically changed its self.
Catalysts lower the activation energy, allowing more successful collisions and a faster rate of reaction I will not be using this factor is my investigation but I will ensure my apparatus is clean accurately from any unwanted substances that may affect my experiment. Concentration Increasing the concentration of solutions will increase reaction rate because more particles are present in the same volume, so they are closer together and will collide more often to react. When the solution is diluted with more water the solute particles are more spread out and so less likely to collide and react.
Also by having a higher concentration there is a greater chance of having more successful collisions. I will be alternating the concentrations of hydrochloric acid to see de how the rate of the reaction is affected In a higher concentration of the reactant particles are more closely packed together. It is more likely that they will collide and a more successful collision will occur. I will be using this factor as it is the major part of my experiment as because I will be changing the concentration of hydrochloric acid to see how the rate of reactions changes with the magnesium ribbon. Surface area.