We can express this as 2 half reactions, one showing the movement of electrons in the magnesium, and the other with the hydrochloric acid. I repeated all 5 concentrations three times to make sure that they were reliable results and in all cases the higher the concentration the higher the rate of reaction. If you include dairy in your diet, that's another source, too. I decided to use the concentration of acid as my variable. The rate of gas bubbles The independent variables Increasing concentration of hydrochloric acid: This will be changed by changing dilution factor.
The magnesium displaces the hydrogen in the acid, so it forms magnesium chloride and hydrogen gas. All chemical reactions involve reactants which when mixed may cause a chemical reaction which will make products. In conclusion, this experiment was successful in determining the relationship between temperature and reaction rate. Activation energy is the minimum amount of energy that particles require for a successful collision resulting in a reaction. Other than those questionable factors, the experiment went smoothly. Therefore, we sought to test the duration of reaction of equal lengths Magnesium ribbons with reducing concentrations of hydrochloric acid.
This is basically how hard and how often particles collide with each other. I could also change the acid reactant to sulphuric acid or phosphoric acid to see and compare the results with different molecular make-ups. I have already stated this in my prediction had stated this in my prediction. The other variables are the temperature of the acid at the beginning, the volume of acid, the surface area of the magnesium strip, the length of the magnesium strip and if the magnesium strip is cleaned or not. There are four main factors which affect the rate of reaction.
This could be due to the number of molecules of hydrochloric acid being proportional to the concentration. This is because there are a greater number of industries in city than in the countryside. Therefore, this study intends to investigate the effect of concentration and surface area of reactants on the rate of chemical reactions. Clark 2002 explains that, finely divided chemical solids have greater surface area than chemical solids in lumps. Thus, this light could have increased the energy of the particles participating in the reaction, and thus increase the inaccuracy because this is an external factor affecting the rate of reaction. In conclusion, although there were some errors associated with this experiment, it was successful in determining the relationship between temperature and reaction rate. Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen.
Similarly, the duration of reaction will be determined using equivalent weights of powdered Magnesium metal. Reaction rate between magnesium ribbon and hydrochloric acid Essay Sample Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. The collision energy depends directly on the kinetic energy of colliding particles, and temperature is a measure of the average kinetic energy of the particles in a substance. The experiment will be carried out at room temperature 25 0C The study variables are summarized in the table below: Variables Operationalization of variables The dependent variables The duration of reaction, time taken for Magnesium to dissolve in hydrochloric acid completely measured using a stopwatch in seconds. Apart from the last result, the results obtained show that as concentration increases, the time taken to displace 50cm3 of water decreases.
In addition, impurities may form on the surface of the magnesium metal therefore, slowing further the rate of reaction. There are certain factors that can affect the rate of reaction. The process was repeated for one more trial. To find percent error, I took the absolute value of the true value minus my calculated value divided by the true value and multiplied by 100%. The mixture should begin to effervesce.
As from 3 sets of readings, an average can be calculated which will provide a more reliable result as it is based upon 3 readings, not just the one reading which may be wrong. From the point the magnesium is added, start the stopwatch, as soon as the effervescing stops, the reaction is over: Magnesium + hydrochloric acid à magnesium chloride + hydrogen All variables of the concentration should be done at room temperature for consistency. This is a polynomial relationship, which implies that the rate of reaction increases exponentially in relation to the increase in temperature. If you don't feel any relief after several rounds of trying, you might have too little hydrochloric acid. Add 40ml of distilled water for dillution.
If you feel immediate burning, you might have too much hydrochloric acid. It is more likely to occur in areas, where there is more pollution. The aqueous vapor pressure was found using a chart. Each experiment run will need 50 cm 3. I think this because of the Collision theory. We also predict that reaction of powdered Magnesium metal with highest concentration of hydrochloric acid will take the shortest duration of reaction.
It is best if the students work in pairs because setting up and starting the experiment requires more than one pair of hands. This demonstration may also be performed using a document projector if a dark background is used. A healthy stomach has a balanced amount of hydrochloric acid in it at all times. Following this, the tip of a buret was calibrated and this volume was recorded. All chemical reactions involve reactants which when mixed may cause a chemical reaction which will make products.
Even after disappearance of magnesium ribbon, gas bubbles were evident, implying the reaction was incomplete. I also said that I thought the reaction doubles with the concentration, but I found out from the gradients that it approximately quadruples when the concentration doubles. According to the collision theory, there are four factors, which affect the rate of reactions; temperature, catalyst, surface area and concentration. While it breaks down protein, it also protects you by forming a barrier that kills micro-organisms before they can make you sick. In a solution of 0. For the Internet I got help from www.