Increasing 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. Using this information, a small piece of metal magnesium is reacted with hydrochloric acid. Similarly, the duration of reaction will be determined using equivalent weights of powdered Magnesium metal. In further investigation to keep this variable controlled would be to have the temperature of the HCl tested with a thermometer before the acid is combined with the magnesium. Acid-Base Reactions Determining Acid Strength Using Magnesium Description: Reaction of an acid with Mg generates H 2 gas. Materials: Mg ribbon 3 Petri dishes 1.0 M HCl 1.0 M boric acid 1.0 M acetic acid Procedure: 1. In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. 2. 18.3 g B. 200 cm 3 of 2 mol/dm 3 hydrochloric acid and ... swirl once to ensure the magnesium is fully coated in the acid. Then measured the temperature after experiment. (2002). Place a Styrofoam cup into a 250 mL beaker as shown in Figure 1. 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. A gaseous product is collected in a long, thin graduated glass tube, called a eudiometer, by displacement of a liquid, usually water. Why does the amount of hydrogen produced per second decrease with time?? I need 2 explanations: First of all why is the reaction exothermic? The volume of hydrogen gas produced is measured over a few minutes, and the results are used to plot a graph This is intended as a class practical. Prediction 1. Reset your stopwatch, a repeat steps 9, 10 and 11 for the subsequent acids. In my case the reactants are hydrochloric acid and magnesium ribbon. However, Barrans (2012) highlights that the reaction rate between magnesium metal and HCl follows first order kinetics. 2 0 obj Empty the beaker and rinse it out. Record the reaction time in a table like Table 1 (below). x��][o\9r~��p�7���;�f��س�� �@F��An˲6�e�ۙ������s�wˁ�`�&Y�*���x>>;k��y�D�T�5���עne�x���?W�v��峳�QTBV/�>;hS�J�ʵ���zyO �t�͖pV7��1��gg�����\���>W����x{���kd�߭�����^�볳?����}�m��!oB6u�=�*2� Then ready with the stopwatch we tipped the magnesium in to beaker and put in the cork with the rubber tubing and started the stopwatch. Powdered solids produces rapid reactions than the same solids in single lumps. In this experiment the reaction between hydrochloric acid solution and magnesium ribbon is used to investigate the effect of reactant concentration on the rate of reaction. Put one piece of magnesium into the beaker of hydrochloric acid, and time the reaction. Cumulative average of reaction duration of: THE EFFECT OF SURFACE AREA ON REACTION RATES. Add up the weights of the five 10 cm-long magnesium ribbons and obtain the average weight in grams. Apparatus 50 mL graduated cylinder hydrochloric acid, HCl, solution balance magnesium, Mg PROCEDURE 1. Discard all the chemicals, wash, and rinse the conical flasks ready for another procedure. He identified the gas as being hydrogen. Therefore, this study intends to investigate the effect of concentration and surface area of reactants on the rate of chemical reactions. For the first experiment we measured in a measuring cylinder 50cm3 of hydrochloric acid and poured it into the beaker. The balanced formula for this is: Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen. New York: Oxford University Press. I am reacting different masses of Magnesium with hydrochloric acid to find the temperature change. The balanced chemical equation for this reaction is Mg (s) + 2 HCl (aq) produces MgCl 2 (aq) + H 2 (g), where the letter "s" stands for solid, "g" is gas and "aq" represents an aqueous solution. Therefore, we sought to test the duration of reaction of equal lengths Magnesium ribbons with reducing concentrations of hydrochloric acid. Therefore, we sought to test the duration of reaction of equal lengths Magnesium ribbons with reducing concentrations of hydrochloric acid. In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. In addition, impurities may form on the surface of the magnesium metal therefore, slowing further the rate of reaction. <> %PDF-1.7 Therefore, the errors were unidirectional therefore consistent. Figure 1: Experimental set-up of HCl-Magnesium reaction. 1�6��ԗ�EF\��ۚ�%|���`z��Z�J*R�J����d�I�;r�s����jO��t^W�t��v�WQ�fk� ƽ����n�D>���$%(��՘�����O���� �qL�!�Y���j�P��*MD[r����[=�C��r Q��c ���w��d��V7W�ڮy�E=�pwG+@ن2w�o�}v{J�ڴ�& 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. The balanced formula for this is: Mg (s) + 2HCL (aq) MgCl2 (aq) + H2 (g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen Record the reaction time in a table like Table 1 (below). Factors That Affect Reaction Rates - Chemwiki 2015. The balanced formula for this is: Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen. Monitor the reaction progress closely and stop your running stopwatch when the Magnesium ribbon completely dissolves in the acid and record the reaction duration in seconds in a data sheet. In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. Secondly, why does the difference in temperature increase as the mass of magnesium increases? High concentrations imply that more reacting molecules are at high proximity to each other therefore intermolecular collisions are frequent therefore forming products frequently. • The gas produced was collected in a gas syringe (as shown opposite) so that its volume could be measured. 4 0 obj The formula equation for this experiment is: Mg + 2HCl MgCl2 + H2 The word Equation for this experiment is: Magnesium + Hydrochloric acid Magnesium Chloride + Hydrogen (s) (aq) (aq) (g) Magnesium will react with hydrochloric acid, because it is higher in the reactivity series that hydrogen. The data you obtain will enable you to answer the question: The Reaction of Magnesium with Hydrochloric Acid In this experiment you will determine the volume of the hydrogen gas that is produced when a sample of magnesium reacts with hydrochloric acid. Chemicals and Reagents Similarly, the duration of reaction will be determined using equivalent weights of powdered Magnesium metal. The volume of the hydrogen gas produced will be measured at room temperature and pressure. In this experiment you will determine the volume of the hydrogen gas which is produced when a sample of magnesium reacts with hydrochloric acid. The study variables are summarized in the table below: Table 1 A table of study variables and operationalization of the study variables. I was suggested to use 20cm3 of hydrochloric acid and 5cm of cleaned magnesium ribbon, and take the volume of hydrogen in the syringe every 10 seconds for the preliminary experiment to. The ratio of the cumulative reaction duration above gives 104.8 sec/58.8 sec = 1.78. The volume of the hydrogen gas produced will be measured at room temperature and pressure. During the reaction, the water bath in the gas delivery system showed gas bubbles ascending to the gas cylinder. The formula is: Mg + 2HCl → MgCl2 + H2(g) - What is the mass in grams of two moles of HCl? The flammability of hydrogen gas can be demonstrated by carefully holding a match or fireplace lighter up to the popping … However, the experimentation had the following inconsistencies as shown the table below. Magnesium will react with hydrochloric acid, because it is higher in the reactivity series than hydrogen. Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. Experiment 5 Reaction of Magnesium with Hydrochloric Acid OUTCOMES After completing this experiment, the student should be able to: develop a procedure for generating and measuring a gas in a reaction. endobj The reaction is represented by the equation Mg (s) + 2HCl (aq) –> MgCl 2 (aq) + H 2 (g). Website. This single replacement reaction is a classic example of a metal reacting in an acid to release hydrogen gas. 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. In the reaction between hydrochloric acid and magnesium, the hydrochloric acid will dissolve the magnesium and produce hydrogen gas. 36.5 g C. 73.0 g D. 82.6 g It is quite reactive giving vigorous reactions towards acids. Magnesium metal (in form of a ribbon or powder) reacts with acids rapidly than water liberating hydrogen gas. A 3 0 obj A table of results showing HCl-Magnesium ribbon reaction duration (seconds) in reducing concentration, Table 3. 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. Retrieved March 8, 2012, from chemguide.co.uk: http://www.chemguide.co.uk/physical/basicrates/surfacearea.html, Gallagher, R., & Ingram, P. (2001). Place about 5cm depth of the acid in each of the five test tubes; Place a small piece of each of the three metals above. This bibliography was generated on Cite This For Me on Thursday, March 26, 2015. These are the sources and citations used to research Magnesium and Hydrochloric Acid Experiment. I tried this but the reaction happened very quickly and the results of the volume of hydrogen were very spread out. Given that, powdered Magnesium metal has a high surface area than equivalent lengths of Magnesium ribbon, we predict that the former will have shorter duration of reaction with hydrochloric acid than the latter. In-text: (Factors That Affect Reaction Rates - … In the zinc and hydrochloric acid experiment the learners collect gas in a balloon. Magnesium ribbon = 37+51+77+158+201/S = 104.8 sec Table 2. In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. For the 10 cm magnesium metal used, there was slight variation in weight. Does the mass of the beaker stay the same explain why? Importantly, suitable acid-base indicators can be used to detect the end of the reaction accurately. 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. Stop the watch when all the magnesium disappears. Stronger acids produce more H 2 bubbles as Mg dissolves in the acidic solution. A constant amount of excess HCl is reacted with varying amounts of magnesium solid. In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. Chemistry for higher tier: New coordinated science. 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. To measure the effect of concentration on the average rate of a reaction. The Reaction of Magnesium with Hydrochloric Acid. The hydrochloric acid appeared to be clear liquid and looked very similar to rubbing alcohol. Choose only one indicator that signifies end of reaction. This bibliography was generated on Cite This For Me on Thursday, March 26, 2015. <>/ExtGState<>/XObject<>/ProcSet[/PDF/Text/ImageB/ImageC/ImageI] >>/MediaBox[ 0 0 595.32 841.92] /Contents 4 0 R/Group<>/Tabs/S>> In acid-base chemical reactions, there are four main variables, which influence the rate of reaction. t��V�+��!N�37v���t�>��ꊘz��7����׵h��LJͻ��^�=�M������i�W��VT�%��t��OM�t�+ge���A��֑�-��k���r7��ru�{��D���BW]����k�����O����:�3̤�jC��t$�&C 5(��ݬMrC5����"7��HΉ����QQ9�jqbZ#$��m[9��jD�M��OW�ۇ��m���n��θ�I��4Nzt�����lk/G�_�H����W��׸y1�X}���'�c������n)kF��9!W���@�WO-e%d-��\b��ru��՘��[1-����xqZrDg��=��X�Z��i�Ҷs��]�8�ΒJ�m;g$ 2�� Magnesium, zinc and iron also react with sulfuric acid. Add 40 ml of distilled water and label the conical flask with the concentration of the HCL poured. I hope this was helpful. Before starting the investigation, I decided to do some research about magnesium and hydrochloric acid. 2. Magnesium reacts with hydrochloric acid according to the equation: Mg(s) + 2 HCl(aq) --> MgCl 2 (aq) + H 2 (g) This demonstration can be used to illustrate the characteristic reaction of metals with acid, a single replacement reaction, or to demonstrate the generation of hydrogen gas. Barrans, R. E. (2012, March). 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. Since magnesium has only one valence and it reacts easily with HCl, it’s easy to generalize to other metals and acids. Pick one piece of Magnesium ribbon drop in the first prepared acid in the conical flask and immediately start your stopwatch. Graph 1: Rate-reaction trends of magnesium metal ribbon and powder with increasing concentration of HCl, Calculations develop a relationship between the mass of magnesium reacted and the volume of … First, repair your working bench by simply removing unnecessary materials. The balanced formula for this is: Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen The chemical equation for this experiment is: Mg (s) + 2 HCl (aq) --> MgCl 2 (aq) + H 2 (g). The volume of the hydrogen gas produced will be measured at room temperature and pressure. 3 cm of magnesium ribbon typically has a mass of 0.04 g and yields 40 cm 3 of hydrogen when reacted with excess acid. 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