Aim: My aim is to find out if heating the hydrochloric acid affects the rate of magnesium and hydrochloric acid. Show
Prediction: I predict that the heating the hydrochloric acid will effect it as heating is one type of changing the rate of reaction. Method: Get three clamps and clamp stands from the cupboard, and set them up and get a water bath and set it up to the right temperature (20-80) and then let it get to the right temp get a gas syringe form…show more content… In a chemical reaction no mass is lost, when the reactants turn in to the product of the reaction, chemical reactions involve a permanent change not just a temporary one. For this to happen their hast to be a change in energy as reactions always give out or take in energy most of the time this is heat energy this means the temperature in a reaction will go up or down. Visible changes can occur in the reaction mixture. These show that a reaction has taken place, for example a gad is given off or a solid is made or the colour changes. Oxidation this happens with most substances usually forming an oxide Exothermic (give out heat) the reaction supplies the energy as heat. Temperature by changing the temperature in a experiment you are effecting the rate of reaction by heating it you are making the experiment go faster because you are making the particles react faster giving a higher chance of a collision happing and if you drop you are causing the Aim: To investigate the effect of temperature on the reaction rate of hydrochloric acid and magnesium. In acid-base chemical reactions, there are four main variables, which influence the rate of reaction. These include the presence or absence of catalyst, temperature, concentration, and surface area of reactants. Temperature influences the rates of reaction through kinetic energy, such that high temperatures increase the kinetic energy of reacting molecules therefore causing frequent collisions, which form products faster. High concentrations imply that more reacting molecules are at high proximity to each other therefore intermolecular collisions are frequent therefore forming products frequently. Reactants with high surface area provide a greater binding surface for other reacting molecules, and therefore increase the number of successful collisions at any moment. To measure, the effect of each of above factors, one has to hold some factors constant during rate reaction experimentation. Therefore, this study intends to investigate the effect of concentration and surface area of reactants on the rate of chemical reactions. Magnesium metal (in form of a ribbon or powder) reacts with acids rapidly than water liberating hydrogen gas. For stance, magnesium metal reacts with hydrochloric to form magnesium chloride salt while displacing hydrogen from the acid as hydrogen gas. This is as shown in the equation below: 2HCl (aq) + Mg (s) => MgCl2 (aq) + H2 (g) Research Question: If magnesium ribbon is replaced with an equivalent weight of powered magnesium, does the rate of reaction between magnesium and hydrochloric acid double? Aims and objectives of the experimentThe 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. Therefore, we sought to test the duration of reaction of equal lengths Magnesium ribbons with reducing concentrations of hydrochloric acid. Similarly, the duration of reaction will be determined using equivalent weights of powdered Magnesium metal. The experiment will be carried at a room temperature 25 0C. Study Variables
The study variables are summarized in the table below: VariablesOperationalization of variablesThe dependent variablesThe duration of reaction, (time taken for Magnesium to dissolve in hydrochloric acid completely) measured using a stopwatch in seconds.The rate of gas bubblesThe independent variablesIncreasing concentration of hydrochloric acid: This will be changed by changing dilution factor.Surface area of Magnesium ribbon: This will be changed by using Magnesium ribbons and powdered Magnesium metal in separate experiments.The constants (controlled variables)The quantity of Magnesium metal used will be held constant by way of using equal lengths of Magnesium ribbons and equivalent weights (in grams) of powdered Magnesium metal.All the reaction will be carried out under a constant temperature (room temperature of 25 0C).
Table 1 A table of study variables and operationalization of the study variables Prediction Hypothesis: Powdered Magnesium metal will reduce the reaction duration by a half if used in place of equivalent length of magnesium ribbon, when reacted with hydrochloric acid. Equipment and MaterialsChemicals and Reagents
Apparatus and personal protection equipment
Experimentation proceduresThe experiment procedure was divided into two related investigations involving equal lengths of Magnesium ribbons and equal amounts of powdered Magnesium metal.
Figure 1: Experimental set-up of HCl-Magnesium reaction Results and ObservationsDuring the reaction, the water bath in the gas delivery system showed gas bubbles ascending to the gas cylinder. At higher acid concentration, the rates of bubble forming were rapid than those in lower acid concentrations were. The most rapid gas bubbles were observed in the acid reactions with powdered Magnesium metal. The duration of reactions were recorded as shown in tables 2 and 3 below. Concentration of HCl (M)3.02.01.51.00.5Reaction duration (sec)375177158201Table 2. A table of results showing HCl-Magnesium ribbon reaction duration (seconds) in reducing concentration Table 3. A table of results showing HCl-Magnesium powder reaction duration (seconds) in reducing concentration Processing and Presenting DataGraph Graph 1: Rate-reaction trends of magnesium metal ribbon and powder with increasing concentration of HCl Calculations Discussion and ConclusionsFrom the experimentation the aims of the experimentation have been achieved. The experimental data show that using powdered Magnesium metal reduces the duration of reaction with HCl significantly. Although we had predicted and hypothesized that the duration of the reaction would be reduced by a half, the data partially supported the hypothesis since the data was 89.1% close to what we predicted. Clark (2002) explains that, finely divided chemical solids have greater surface area than chemical solids in lumps. Powdered solids produces rapid reactions than the same solids in single lumps. However, Barrans (2012) highlights that the reaction rate between magnesium metal and HCl follows first order kinetics. This is because the hydrogen ions (H+) from the acid I have a large binding surface on magnesium metal but later, the surface area diminishes due to other factors in the reaction. For instance hydrogen bubbles block magnesium surface or blow the magnesium to the surface of the acid solution therefore, slowing down the reaction. In addition, impurities may form on the surface of the magnesium metal therefore, slowing further the rate of reaction. Similarly, Gallagher & Ingram (2001) say that the depletion of H+ during the reaction of magnesium and HCl is factor that slows down the reaction as time goes on. Therefore, considering concentration factor and surface are factor of reactants it is evident that the rate reaction curve trends would not be linear as expected, but rather exponential. Data EvaluationThe experimentation procedures followed were standard for all the two sets of experiments conducted, including data collection mode. Given that, the experiment was carried out under the same conditions, the data obtained are reliable and generalizable. However, the experimentation had the following inconsistencies as shown the table below. What would happen to the temperature during the reaction between magnesium and hydrochloric acid?Burning magnesium is an exothermic reaction because when magnesium and oxygen particles collide to form new bonds, energy is released into the surroundings. Citric acid and baking soda is an endothermic reaction as the temperature decreases. Magnesium and hydrochloric acid is exothermic as the temperature increases.
How does temperature of hydrochloric acid affect the reaction rate?As the temperature increases, the particles gain kinetic energy and move faster. This means that at higher temperatures, the particles collide more often and with more energy. Thus, increasing the temperature will increase the rate of reaction.
What factors affect the rate of reaction between magnesium and hydrochloric acid?In a reaction between magnesium metal and hydrochloric acid, magnesium atoms must collide with the hydrogen ions. When the magnesium atoms form one big lump... the number of collisions per second between magnesium and hydrogen is higher, and the rate of reaction is faster.
How to increase the rate of reaction between magnesium and hydrochloric acid?Grinding up the magnesium into a powder increases the surface area, so the acid has more space to react on. This means the larger surface area, the quicker reaction time. Magnesium reacts very strongly with hydrochloric acid.
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