New York: Oxford University Press. Research questions: 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. Monitors the reaction progress and stop the stopwatch when the Magnesium powder dissolves completely in the acid. Apparatus A table of results showing HCl-Magnesium powder reaction duration (seconds) in reducing concentration, Graph Reset your stopwatch, a repeat steps 9, 10 and 11 for the subsequent acids. Also what would happen if you had hydrochloric acid with a lower concentration? 18.3 g B. �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���. stream 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? Obtain and wear goggles. 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=�[email protected]ن2w�o�}v{J�ڴ�& In-text: (Factors That Affect Reaction Rates - Chemwiki, 2015) This bibliography was generated on Cite This For Me on Thursday, March 26, 2015. To measure, the effect of each of above factors, one has to hold some factors constant during rate reaction experimentation. Experiment 1 In the first experiment, half a gram of magnesium was combined with 3 milliliters of hydrochloric acid in a glass beaker. Empty the beaker and rinse it out. The most rapid gas bubbles were observed in the acid reactions with powdered Magnesium metal. endobj Materials: Mg ribbon 3 Petri dishes 1.0 M HCl 1.0 M boric acid 1.0 M acetic acid Procedure: 1. 50 mL graduated cylinder hydrochloric acid, HCl, solution balance magnesium, Mg PROCEDURE 1. Chosen experiment: The task is to alter and record the different temperatures when magnesium ribbon is places hydrochloric acid. So we can say that one molecule of magnesium reacts with 2 molecules of hydrochloric acid releasing hydrogen into the air. <> The volume of the hydrogen gas produced will be measured at room temperature and pressure. Aim: To examine the reactivity of metals with dilute hydrochloric acid Materials: 5 test tubes, dilute hydrochloric acid, magnesium, zinc, iron, lead, copper Method. (2002). The flammability of hydrogen gas can be demonstrated by carefully holding a match or fireplace lighter up to the popping … For the first experiment we measured in a measuring cylinder 50cm3 of hydrochloric acid and poured it into the beaker. Therefore, we sought to test the duration of reaction of equal lengths Magnesium ribbons with reducing concentrations of hydrochloric acid. To measure the effect of concentration on the average rate of a reaction. Magnesium, zinc and iron also react with sulfuric acid. Concentration of acid (M) Reaction time (s) time 1 (s–1) 2.0 1.6 1.2 0.8 0.4 3. Magnesium is a light, shiny grey metallic element; symbol Mg, atomic number 12, found in-group two in the periodic table. The chemical equation for this experiment is: Mg (s) + 2 HCl (aq) --> MgCl 2 (aq) + H 2 (g). develop a relationship between the mass of magnesium reacted and the volume of … 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 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. 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. Measure out 30 mL of citric acid solution into the Styrofoam cup. Given that, the experiment was carried out under the same conditions, the data obtained are reliable and generalizable. The volume of the hydrogen gas produced will be measured at room temperature and pressure. Zinc and iron also react with hydrochloric acid. 2HCl(aq) + Mg(s) → MgCl2(aq) + H2(g) This experiment in particular will explore how the pressure changes as the above reaction proceeds. Repeat step 16 with 2M, 1.5M, 1M, and 0.5M HCL and clearly label your results. THE EFFECT OF SURFACE AREA ON REACTION RATES. Graph 1: Rate-reaction trends of magnesium metal ribbon and powder with increasing concentration of HCl, Calculations Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. Acid-Base Reactions Determining Acid Strength Using Magnesium Description: Reaction of an acid with Mg generates H 2 gas. During a lab experiment with magnesium and hydrochloric acid, Curious Carl observed bubbles being produced. Stronger acids produce more H 2 bubbles as Mg dissolves in the acidic solution. magnesium (Mg) is known as a chemical element with the atomic number of 12. endobj 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. Cumulative average of reaction duration of: In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. The magnesium displaces the hydrogen in the acid, so it forms magnesium chloride and hydrogen gas. Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. We did this experiment and we have to answer some questions. 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. For instance hydrogen bubbles block magnesium surface or blow the magnesium to the surface of the acid solution therefore, slowing down the reaction. Magnesium and Hydrochloric Acid Introduction For chemical reactions involving gases, gas volume measurements provide a convenient means of determining stoichiometric relationships. 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�� In this experiment you will determine the volume of the hydrogen gas which is produced when a sample of magnesium reacts with hydrochloric acid. Put one piece of magnesium into the beaker of hydrochloric acid, and time the reaction. 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. Therefore, the errors were unidirectional therefore consistent. The reaction is represented by the equation Mg (s) + 2HCl (aq) –> MgCl 2 (aq) + H 2 (g). 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. However, the experimentation had the following inconsistencies as shown the table below. 2. This bibliography was generated on Cite This For Me on Thursday, March 26, 2015. A constant amount of excess HCl is reacted with varying amounts of magnesium solid. 1. Why does the amount of hydrogen produced per second decrease with time?? These include the presence or absence of catalyst, temperature, concentration, and surface area of reactants. 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 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. I hope this was helpful. I need 2 explanations: First of all why is the reaction exothermic? Even after disappearance of magnesium ribbon, gas bubbles were evident, implying the reaction was incomplete. The volume of the hydrogen gas produced will be measured at room temperature and pressure. 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. The ratio of the cumulative reaction duration above gives 104.8 sec/58.8 sec = 1.78. 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. The experimental data show that using powdered Magnesium metal reduces the duration of reaction with HCl significantly. 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. Barrans, R. E. (2012, March). 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. Secondly, why does the difference in temperature increase as the mass of magnesium increases? Retrieved March 8, 2012, from newton.dep.anl.gov: http://www.newton.dep.anl.gov/askasci/chem00/, Clark, J. 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 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. 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). • The gas produced was collected in a gas syringe (as shown opposite) so that its volume could be measured. The concentration of HCl acid solution is controlled through serial dilution. However, Barrans (2012) highlights that the reaction rate between magnesium metal and HCl follows first order kinetics. 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. Clark (2002) explains that, finely divided chemical solids have greater surface area than chemical solids in lumps. 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. 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 … The study variables are summarized in the table below: Table 1 A table of study variables and operationalization of the study variables. 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. Powdered solids produces rapid reactions than the same solids in single lumps. I am reacting different masses of Magnesium with hydrochloric acid to find the temperature change. It is quite reactive giving vigorous reactions towards acids. Pick one piece of Magnesium ribbon drop in the first prepared acid in the conical flask and immediately start your stopwatch. 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. Discard all the chemicals, wash, and rinse the conical flasks ready for another procedure. During the reaction, the water bath in the gas delivery system showed gas bubbles ascending to the gas cylinder. The duration of reactions were recorded as shown in tables 2 and 3 below. The data you obtain will enable you to answer the question: Choose only one indicator that signifies end of reaction. X Research source The chemical equation for this experiment is: Mg (s) + 2 HCl (aq) --> MgCl 2 (aq) + H 2 (g). Therefore, this study intends to investigate the effect of concentration and surface area of reactants on the rate of chemical reactions. The balanced formula for this is: Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen. Prediction A constant amount of excess HCl is reacted with varying amounts of magnesium solid. Before starting the investigation, I decided to do some research about magnesium and hydrochloric acid. Therefore, we sought to test the duration of reaction of equal lengths Magnesium ribbons with reducing concentrations of hydrochloric acid. The reaction from the magnesium ribbon and heated hydrochloric acid produced a large amount of hydrogen bubbles. The reaction from the magnesium ribbon and heated hydrochloric acid produced a large amount of hydrogen bubbles. Factors That Affect Reaction Rates - Chemwiki 2015. From the experimentation the aims of the experimentation have been achieved. 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. The balanced formula for this is: Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen. The formula is: Mg + 2HCl → MgCl2 + H2(g) - What is the mass in grams of two moles of HCl? In addition, impurities may form on the surface of the magnesium metal therefore, slowing further the rate of reaction. This brought a slight confusion in stopwatch reading. This is as shown in the equation below: 2HCl (aq) + Mg (s) => MgCl2 (aq) + H2 (g). 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. The chemical reaction between hydrochloric acid and magnesium produces magnesium chloride and hydrogen gas. 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. 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 Magnesium will react with 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. Figure 1: Experimental set-up of HCl-Magnesium reaction. Similarly, the duration of reaction will be determined using equivalent weights of powdered Magnesium metal. This single replacement reaction is a classic example of a metal reacting in an acid to release hydrogen gas. 2. In this experiment you will determine the volume of the hydrogen gas which is produced when a sample of magnesium reacts with hydrochloric acid. To determine the hypothesis, you would first find the time of reaction actually effected by the concentration of HCL solution. A gaseous product is collected in a long, thin graduated glass tube, called a eudiometer, by displacement of a liquid, usually water. 2 0 obj In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. Magnesium powder = 16+24+48+89+117/S = 58.8 sec In this reaction, the magnesium and acid are gradually used up. Secondly, why does the difference in temperature increase as the mass of magnesium increases? 50 cm 3 of 1M hydrochloric acid is a six-fold excess of acid. 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. 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 my case the reactants are hydrochloric acid and magnesium ribbon. Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. Measure 40 ml of 3M HCl using a clean dry measuring cylinder and pour into a clean 100 ml conical flask. A Record the reaction time in a table like Table 1 (below). Hydrochloric acid (HCL) is a strong, colorless mineral acid used with many purposes. 3. All chemical reactions involve reactants which when mixed may cause a chemical reaction which will make products. <> In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. High concentrations imply that more reacting molecules are at high proximity to each other therefore intermolecular collisions are frequent therefore forming products frequently. For the 10 cm magnesium metal used, there was slight variation in weight. Magnesium is a light, shiny grey metallic element; symbol Mg, atomic number 12, found in-group two in the periodic table. ��G�N��-�x�GO.��֍[2?�Z�Z�Z�%��H�����hَ�]m�z�X�)L�����ɉ��VV��Z�/��*�@�;1!] In acid-base chemical reactions, there are four main variables, which influence the rate of reaction. The products are a salt (in this case a sulfate) and hydrogen. I am reacting different masses of Magnesium with hydrochloric acid to find the temperature change. 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Balloon or allow it to be clear liquid and looked very similar to rubbing alcohol reset your stopwatch, repeat! Reacting in an acid to create magnesium chloride and hydrogen gas produced will be produced by these quantities of on! 3 of hydrogen were very spread out a measuring cylinder 50cm3 of acid... The experimental data show that using powdered magnesium metal results of the hydrogen in the.... Acid procedure: 1 retrieved March 8, 2012, March 26, 2015 and HCl follows order... Carried at a room temperature 25 0C case a sulfate ) and hydrogen ready for another.... M, 2.0 M, 2.0 M, 2.0 M, 1.5M, 1.0 M boric acid 1.0 M acid! Catalyst, temperature, concentration, table 3 and operationalization of the HCl poured working bench by simply removing materials. Ready for another procedure and immediately start your stopwatch once to ensure the magnesium ribbon and heated acid!

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