X Research source The chemical equation for this experiment is: Mg (s) + 2 HCl (aq) --> MgCl 2 (aq) + H 2 (g). Barrans, R. E. (2012, March). Therefore, we sought to test the duration of reaction of equal lengths Magnesium ribbons with reducing concentrations of hydrochloric acid. The weight inconsistencies were small therefore, a low significance error, Use at least two sets of experiment to get average of results to minimize the impact of experimental errors. During a lab experiment with magnesium and hydrochloric acid, Curious Carl observed bubbles being produced. 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. <> I tried this but the reaction happened very quickly and the results of the volume of hydrogen were very spread out. Make sure you put on your personal protective clothing and safety goggles. This bibliography was generated on Cite This For Me on Thursday, March 26, 2015. The Reaction of Magnesium with Hydrochloric Acid KEY In this experiment you will determine the volume of the hydrogen gas that is produced when a sample of magnesium reacts with hydrochloric acid. In this experiment you will determine the volume of the hydrogen gas which is produced when a sample of magnesium reacts with hydrochloric acid. Aim: To examine the reactivity of metals with dilute hydrochloric acid Materials: 5 test tubes, dilute hydrochloric acid, magnesium, zinc, iron, lead, copper Method. Given that, the experiment was carried out under the same conditions, the data obtained are reliable and generalizable. Prediction The magnesium is a solid that reacts with the aqueous hydrochloric acid to form hydrogen gas and aqueous magnesium chloride. The data you obtain will enable you to answer the question: In the zinc and hydrochloric acid experiment the learners collect gas in a balloon. 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� The reaction from the magnesium ribbon and heated hydrochloric acid produced a large amount of hydrogen bubbles. We did this experiment and we have to answer some questions. Cumulative average of reaction duration of: 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. Put one piece of magnesium into the beaker of hydrochloric acid, and time the reaction. 200 cm 3 of 2 mol/dm 3 hydrochloric acid and ... swirl once to ensure the magnesium is fully coated in the acid. Factors that influence rates of reactions include change in concentration, temperature, surface area, or the addition of a catalyst. • The gas produced was collected in a gas syringe (as shown opposite) so that its volume could be measured. Measure out 30 mL of citric acid solution into the Styrofoam cup. Determination of end of reaction was sometimes uncertain. %���� This is as shown in the equation below: 2HCl (aq) + Mg (s) => MgCl2 (aq) + H2 (g). I need 2 explanations: First of all why is the reaction exothermic? Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. I am reacting different masses of Magnesium with hydrochloric acid to find the temperature change. Why does the amount of hydrogen produced per second decrease with time?? In-text: (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. The change in pressure in a constant-volume (500-mL Erlenmeyer … The experiment will be carried at a room temperature 25 0C. 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. develop a relationship between the mass of magnesium reacted and the volume of … The duration of reactions were recorded as shown in tables 2 and 3 below. This is a low significance error since we based mostly on the disappearance of magnesium into the acid rather than disappearance gas bubbles. Measure 40 ml of 3M HCl using a clean dry measuring cylinder and pour into a clean 100 ml conical flask. For the first experiment we measured in a measuring cylinder 50cm3 of hydrochloric acid and poured it into the beaker. The chemical reaction between hydrochloric acid and magnesium produces magnesium chloride and hydrogen gas. 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. 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. These include the presence or absence of catalyst, temperature, concentration, and surface area of reactants. 2. Zinc and iron also react with hydrochloric acid. 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. Cut 5 equal sizes (10 cm) pieces of Magnesium from the fleshly cleaned Magnesium ribbon, weigh each of them using a digital weighing balance and record their weights. The chemical reaction between hydrochloric acid and magnesium produces magnesium chloride and hydrogen gas. 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? Experiment 1 In the first experiment, half a gram of magnesium was combined with 3 milliliters of hydrochloric acid in a glass beaker. Similarly, the duration of reaction will be determined using equivalent weights of powdered Magnesium metal. Record the reaction time in a table like Table 1 (below). THE EFFECT OF SURFACE AREA ON REACTION RATES. Concentration of acid (M) Reaction time (s) time 1 (s–1) 2.0 1.6 1.2 0.8 0.4 3. Using the sum of partial pressures rule and the ideal gas law to find moles, the molar mass of Mg (s) can be calculated only knowing the pressure of H 2 (g). magnesium (Mg) is known as a chemical element with the atomic number of 12. The time taken for the magnesium to totally dissolve in the hydrochloric acid was recorded by a stopwatch started as the magnesium ribbon was dropped into the hydrochloric acid inside the beaker. The experimental data show that using powdered Magnesium metal reduces the duration of reaction with HCl significantly. The reaction from the magnesium ribbon and heated hydrochloric acid produced a large amount of hydrogen bubbles. Do not light the gas in the balloon or allow it to be near flame. ��G�N��-�x�GO.��֍[2?�Z�Z�Z�%��H�����hَ�]m�z�X�)L�����ɉ��VV��Z�/��*�@�;1!] There will be an explosion. A constant amount of excess HCl is reacted with varying amounts of magnesium solid. Place a Styrofoam cup into a 250 mL beaker as shown in Figure 1. The rate of reaction of magnesium with hydrochloric acid Magnesium reacts with dilute hydrochloric acid in a conical flask which is connected to an inverted measuring cylinder in a trough of water. Similarly, the duration of reaction will be determined using equivalent weights of powdered Magnesium metal. In my case the reactants are hydrochloric acid and magnesium ribbon. 50 mL graduated cylinder hydrochloric acid, HCl, solution balance magnesium, Mg PROCEDURE 1. <> The balanced chemical equation is: Mg_((s))+ 2HCl_((aq))rarrMgCl_(2(aq)) + H_(2(g) The reaction between magnesium and hydrochloric acid combine to form a salt of magnesium chloride and release hydrogen gas. In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. The following chemicals and reagents were required in the experimentation: Apparatus and personal protection equipment. Pick one piece of Magnesium ribbon drop in the first prepared acid in the conical flask and immediately start your stopwatch. Retrieved March 8, 2012, from chemguide.co.uk: http://www.chemguide.co.uk/physical/basicrates/surfacearea.html, Gallagher, R., & Ingram, P. (2001). <> Magnesium will react with hydrochloric acid, because it is higher in the reactivity series than hydrogen. <>/ExtGState<>/XObject<>/ProcSet[/PDF/Text/ImageB/ImageC/ImageI] >>/MediaBox[ 0 0 595.32 841.92] /Contents 4 0 R/Group<>/Tabs/S>> Analyzed our informations and datas to compare to other group's datas. Therefore, we sought to test the duration of reaction of equal lengths Magnesium ribbons with reducing concentrations of hydrochloric acid. So we can say that one molecule of magnesium reacts with 2 molecules of hydrochloric acid releasing hydrogen into the air. Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. A First, repair your working bench by simply removing unnecessary materials. In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. The balanced formula for this is: Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen. Clark (2002) explains that, finely divided chemical solids have greater surface area than chemical solids in lumps. A. In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. Table 2. The Reaction of Magnesium with Hydrochloric Acid. The products are a salt (in this case a sulfate) and hydrogen. Magnesium will react with hydrochloric acid, because it is higher in the reactivity series than hydrogen. The experimentation procedures followed were standard for all the two sets of experiments conducted, including data collection mode. 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. In acid-base chemical reactions, there are four main variables, which influence the rate of reaction. This single replacement reaction is a classic example of a metal reacting in an acid to release hydrogen gas. The balanced formula for this is: Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen. Therefore, we sought to test the duration of reaction of equal lengths Magnesium ribbons with reducing concentrations of hydrochloric acid. 3. Magnesium reacts with hydrochloric 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. Reset your stopwatch timer and prepare a gas delivery system including water bath as shown figure one below. The balanced formula for this is: Mg (s) + 2HCL (aq) MgCl2 (aq) + H2 (g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen Mg (s) + 2HCL (aq) MgCl2 (aq) + H2 (g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen Magnesium will react with hydrochloric acid, because it is higher in the reactivity series than hydrogen. He identified the gas as being hydrogen. Monitors the reaction progress and stop the stopwatch when the Magnesium powder dissolves completely in the acid. endobj The quantities for this experiment are as follows: 1 g of magnesium will require approximately 42 ml of 1M hydrochloric acid to be consumed. Therefore, the errors were unidirectional therefore consistent. 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. Importantly, suitable acid-base indicators can be used to detect the end of the reaction accurately. 3 0 obj This will reduce reaction errors related to impurities. Concentration of acid (M) Reaction time (s) time 1 (s–1) 2.0 1.6 1.2 0.8 0.4 3. Best educational portal - worldwide students help, The duration of reaction, (time taken for Magnesium to dissolve in hydrochloric acid completely) measured using a stopwatch in seconds.The rate of gas bubbles. Standardized hydrochloric acid concentrations (3.0 M, 2.0 M, 1.5M, 1.0 M and 0.5M ). (2002). 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. Describe the materials before and after stating whether they are a metal or non metal. Label the Petri dishes with each acid. A gaseous product is collected in a long, thin graduated glass tube, called a eudiometer, by displacement of a liquid, usually water. Factors That Affect Reaction Rates - Chemwiki 2015. The experiment will be carried at a room temperature 25 0C. Wrap the magnesium pieces immediately in an aluminum foil to prevent them from being re-oxidized. Similarly, the duration of reaction will be determined using equivalent weights of powdered Magnesium metal. 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. Though the room temperature was kept the same throughout the experiment other thing could have affected the temperature of the hydrochloric acid and the magnesium. Repeat step 5 and 6 for 2M, 1.5M, 1M, and 0.5M HCL and keep all the acids ready on the working bench. The volume of the hydrogen gas produced will be measured at room temperature and pressure. Obtain and wear goggles. magnesium (Mg) is known as a chemical element with the atomic number of 12. The experiment will be carried at a room temperature 25 0C. 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. To measure, the effect of each of above factors, one has to hold some factors constant during rate reaction experimentation. This experiment determines the stoichiometry of a reaction of magnesium and HCl by measuring the pressure of the hydrogen gas produced using a PASCO Absolute Pressure Sensor and a PASCO Science Workshop 500 computer interface. In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. 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. Add 40 ml of distilled water and label the conical flask with the concentration of the HCL poured. 1. 1 0 obj The volume of the hydrogen gas produced will be measured at room temperature and pressure. The magnesium displaces the hydrogen in the acid, so it forms magnesium chloride and hydrogen gas. Starter Experiment - Investigating the rate of reaction between Prepare the following solution • Sulphuric acid 2 mol dm 3 You w depend on how much of the solution is used in each experiment and how many to a conical flask. The data you obtain will enable you to answer the question: Magnesium, zinc and iron also react with sulfuric acid. Secondly, why does the difference in temperature increase as the mass of magnesium increases? Add up the weights of the five 10 cm-long magnesium ribbons and obtain the average weight in grams. 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. The ratio of the cumulative reaction duration above gives 104.8 sec/58.8 sec = 1.78. Chosen experiment: The task is to alter and record the different temperatures when magnesium ribbon is places hydrochloric acid… 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. 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. Also what would happen if you had hydrochloric acid with a lower concentration? The chemical equation for this experiment is: Mg (s) + 2 HCl (aq) --> MgCl 2 (aq) + H 2 (g). 4 0 obj 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. I am reacting different masses of Magnesium with hydrochloric acid to find the temperature change. I hope this was helpful. 5 7980 • In two experiments, two equal masses of magnesium ribbon were allowed to react with two 50 cm3portions of dilute hydrochloric acid. Measuring reaction rates Aim. Powdered solids produces rapid reactions than the same solids in single lumps. Graph 1: Rate-reaction trends of magnesium metal ribbon and powder with increasing concentration of HCl, Calculations endobj A 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. A table of results showing HCl-Magnesium ribbon reaction duration (seconds) in reducing concentration, Table 3. Magnesium will react with hydrochloric acid, because it is higher in the reactivity series than hydrogen. 2HCl(aq) + Mg(s) → MgCl2(aq) + H2(g) This experiment in particular will explore how the pressure changes as the above reaction proceeds. Before starting the investigation, I decided to do some research about magnesium and hydrochloric acid. 2. Empty the beaker and rinse it out. The hydrochloric acid appeared to be clear liquid and looked very similar to rubbing alcohol. Magnesium ribbon = 37+51+77+158+201/S = 104.8 sec 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. 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. By inducing a chemical reaction by reacting a strip of magnesium to hydrochloric acid, the time of the hydrogen gas reacted with magnesium can be acquired through a series of calculations. Research questions: The data you obtain will enable you to answer the question: Though the room temperature was kept the same throughout the experiment other thing could have affected the temperature of the hydrochloric acid and the magnesium. Even after disappearance of magnesium ribbon, gas bubbles were evident, implying the reaction was incomplete. Materials: Mg ribbon 3 Petri dishes 1.0 M HCl 1.0 M boric acid 1.0 M acetic acid Procedure: 1. 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. The balanced formula for this is: Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen Magnesium will react with 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. The experiment procedure was divided into two related investigations involving equal lengths of Magnesium ribbons and equal amounts of powdered Magnesium metal. Through this experiment, we have tested the process in which the time of reaction can be acquired through the undertaking of a chemical reaction, in this case, one between hydrochloric acid and magnesium. 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. 18.3 g B. This experiment determines the stoichiometry of a reaction of magnesium and HCl by measuring the pressure of the hydrogen gas produced using a PASCO Absolute Pressure Sensor and a PASCO Science Workshop 500 computer interface. The time taken for the magnesium to totally dissolve in the hydrochloric acid was recorded by a stopwatch started as the magnesium ribbon was dropped into the hydrochloric acid inside the beaker. 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. 50 cm 3 of 1M hydrochloric acid is a six-fold excess of acid. It is quite reactive giving vigorous reactions towards acids. In-text: (Factors That Affect Reaction Rates - … When magnesium and hydrochloric acid react together, they produce hydrogen right? The balanced formula for this is: Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen Before starting the investigation, I decided to do some research about magnesium and hydrochloric acid. The flammability of hydrogen gas can be demonstrated by carefully holding a match or fireplace lighter up to the popping … Discard all the chemicals, wash, and rinse the conical flasks ready for another procedure. Factors That Affect Reaction Rates - Chemwiki 2015. In addition, impurities may form on the surface of the magnesium metal therefore, slowing further the rate of reaction. Apparatus These are the sources and citations used to research Magnesium and Hydrochloric Acid Experiment. %PDF-1.7 Retrieved March 8, 2012, from newton.dep.anl.gov: http://www.newton.dep.anl.gov/askasci/chem00/, Clark, J. Stop the watch when all the magnesium disappears. During the reaction, the water bath in the gas delivery system showed gas bubbles ascending to the gas cylinder. Does the mass of the beaker stay the same explain why? Using this information, a small piece of metal magnesium is reacted with hydrochloric acid. Therefore, this study intends to investigate the effect of concentration and surface area of reactants on the rate of chemical reactions. Magnesium is a light, shiny grey metallic element; symbol Mg, atomic number 12, found in-group two in the periodic table. Becaus… The main substances that were used in the experiment were hydrochloric acid (HCL) and magnesium ribbon(Mg) when these materials combined there was a chemical reaction, the reaction was that there was bubbling and fizzing when the magnesium dissolved, there was a pattern when the temperatures changed, the molecules in the acid would change speed cause the reaction to be either fast or slow, … At higher acid concentration, the rates of bubble forming were rapid than those in lower acid concentrations were. Magnesium powder = 16+24+48+89+117/S = 58.8 sec It is quite reactive giving vigorous reactions towards acids. We also predict that reaction of powdered Magnesium metal with highest concentration of hydrochloric acid will take the shortest duration of 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�& The volume of the hydrogen gas produced will be measured at room temperature and pressure. The magnesium looked like a gray powder. 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. For instance hydrogen bubbles block magnesium surface or blow the magnesium to the surface of the acid solution therefore, slowing down the reaction. The reaction is represented by the equation Mg (s) + 2HCl (aq) –> MgCl 2 (aq) + H 2 (g). I need 2 explanations: First of all why is the reaction exothermic? 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. develop a relationship between the mass of magnesium reacted and the volume of … Since magnesium has only one valence and it reacts easily with HCl, it’s easy to generalize to other metals and acids. The concentration of HCl acid solution is controlled through serial dilution. 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. Hydrochloric acid (HCL) is a strong, colorless mineral acid used with many purposes. 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. Chemicals and Reagents p137. Just more than 900 ml of hydrogen gas will be produced by these quantities of reactants. Choose only one indicator that signifies end of reaction. For the first experiment we measured in a measuring cylinder 50cm3 of hydrochloric acid and poured it into the beaker. 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. Chosen experiment: The task is to alter and record the different temperatures when magnesium ribbon is places hydrochloric acid. Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. Part I Citric Acid plus Baking Soda 2. stream The magnesium is a solid that reacts with the aqueous hydrochloric acid to form hydrogen gas and aqueous magnesium chloride. A constant amount of excess HCl is reacted with varying amounts of magnesium solid. Use the average weight as obtained in 15 above and weigh of an equivalent weight of Magnesium powder (for this case 0.102 grams) and pour into the first conical flask containing the 3 M HCl acid, start your stopwatch, and immediately cork the flask to the gas delivery system. 2 0 obj The real life use for this example in chemistry is that it’s a way to understand metal-acid reactions in general. However, Barrans (2012) highlights that the reaction rate between magnesium metal and HCl follows first order kinetics. �j��?�����2��>2r���I��M��Q�l�����q)T��84�%�W{��i|���A�K� 4`���e�]D�@b�@���J4(�,�԰ k�(K��x�銁�Qth�%����ѽ67�m�VdrD�����վ�����PU�`�\p��+���"�ת-�ب����zf���.����i���v��:������4�ȣ� �픢6k`֑�P�c� �u����Z��v��;E�cE;��X�H���. Secondly, why does the difference in temperature increase as the mass of magnesium increases? This brought a slight confusion in stopwatch reading. In this experiment you will determine the volume of the hydrogen gas which is produced when a sample of magnesium reacts with hydrochloric acid. This bibliography was generated on Cite This For Me on Thursday, March 26, 2015. Aim: To examine the reactivity of metals with dilute hydrochloric acid Materials: 5 test tubes, dilute hydrochloric acid, magnesium, zinc, iron, lead, copper Method. However, the experimentation had the following inconsistencies as shown the table below. In this reaction, the magnesium and acid are gradually used up. Reset your stopwatch, a repeat steps 9, 10 and 11 for the subsequent acids. All chemical reactions involve reactants which when mixed may cause a chemical reaction which will make products. Explains that, finely divided chemical solids have greater surface area than chemical solids have greater surface area chemical! Why does the mass of magnesium with hydrochloric acid and magnesium produces magnesium chloride and hydrogen single! 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Is fully coated in the acid, HCl, it ’ s a way to understand metal-acid in... //Www.Chemguide.Co.Uk/Physical/Basicrates/Surfacearea.Html, Gallagher, R. E. ( 2012, from newton.dep.anl.gov: http: //www.chemguide.co.uk/physical/basicrates/surfacearea.html,,! That the reaction exothermic release hydrogen gas produced will be determined using equivalent weights of powdered magnesium metal and follows... The reaction exothermic using a clean dry measuring cylinder 50cm3 of hydrochloric acid and magnesium ribbon typically has mass! Than those in lower acid concentrations ( 3.0 M, 2.0 M, 1.5M 1M... A lower concentration, R., & Ingram, P. ( 2001.! Experimentation the aims of the hydrogen gas Cite this for Me on Thursday, March.! Quickly and the results of the hydrogen gas ( as shown in 1! Chemicals, wash, and time the reaction happened very quickly and the results of the hydrogen gas be! Hydrogen were very spread out when mixed may cause a chemical element with the concentration of solution... 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