Thermochemistry: An Ice Calorimeter Determination of Reaction Enthalpy D. F. Nachman 6/23/2010 Abstract: An ice calorimeter was used to study the reaction of magnesium metal and 1.00M sulfuric acid solution: Mg(s) + H2SO4(aq) →MgSO4(aq) + H2(g). We found the experimental molar enthalpy of reaction to be ΔH = –355 ± 17 kJ/mol at 0°C‚ 24% lower than the textbook value of ΔH° = –466.9 kJ/mol‚ reported at 25°C. Introduction Whether a chemical reaction occurs spontaneously or is driven by an outside
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Ground calcium carbonate‚ commonly referred to as GCC‚ is primarily based on limestone and chalk in the UK‚ though marble stone is imported and processed at a few locations. Generally‚ the processing includes washing‚ sorting of undesirable contaminants‚ grinding‚ size classification of particles and possibly drying. http://www.crusherindustry.com/index.php/ground-carbonate-calcium-factory-for-sale-uk/ T130x ultrafine grinding mill is a fine powder and ultrafine calcium carbonates powder production
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THE Ksp of Magnesium Oxalate ABSTRACT INTRODUCTION In this experiment the solubility product constant of the salt magnesium oxalate (MgC2O4)will be determined. The system of interest exists as a solid in equilibrium: Precipitation reaction of EXPERIMENTAL METHODS Preparation of the 0.15M Potassium Permanganate (KMnO4) solution {text:list-item} B. Prepare precipitation mixtures 1. Obtain three labeled 20-mL vials from the cart. 2. Burets are set up in the lab with 0.250 M
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Design Objective: Find the standard molar enthalpy of combustion for magnesium. Manipulated Variables- volume of HCl‚ length of magnesium strip‚ mass of magnesium oxide‚ Controlled Variable- type of calorimeter (Styrofoam cup) Responding Variable- change in temperature Procedure: 1. Cut out 3 pieces of magnesium strips each with lengths of maximum 5 centimeters. 2. Measure and record the lengths of the magnesium. 3. Scrub the magnesium strips with steel wool to clean out impurities
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Heat of Combustion of Magnesium Background: The students were given full instructions on how to experimentally determine the enthalpy of reaction (ΔHrxn) for the combustion of magnesium ribbon‚ using Hess’s Law. Data Collection: | |Reaction 1 |Reaction 2 | | |(MgO) |(Mg)
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Measuring the Enthalpy change of combustion Abstract This simple experiment is carried out to show the difference in the enthalpy change of combustion between two fuels‚ hexane and methanol. These fuels are individually weighed before and after used as heat source to heat water in a calorimeter. The result is used to find out amount of heat transferred by the fuel‚ amount of fuel used and the enthalpy change of combustion. Introduction Enthalpy change of combustion is the enthalpy change when
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Determining an Enthalapy Change of Reaction Purpose of Experiment The purpose of this experiment is to determine the enthalapy change for the displacement reaction: Zn(s) + CuSO4(aq) Cu(s) + ZnSO4(aq) Hypothesis With this experiment I can also not make a hypothesis‚ because we did actually not do the experiment‚ but we were told that the temperature would make a sudden drop ‚ but we can measure the ΔT of the surrounding. The reaction is endothermic because the system will take in energy
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Enthalpy of Displacement IB Topic: Energetics Assessment Criteria: DCP‚ CE DATA COLLECTION AND PROCESSING ASPECT MARKS AWARDED Recording raw data: Processing raw data: Presenting Proceeded data: TOTAL: CONCLUSION AND EVALUATION Conclusion Evaluation Improving the procedure TOTAL AIM: Experimentally determine the enthalpy change of the displacement reaction between zinc and copper sulphate. Zn (s) + CuSO4 (aq) Cu (s) + ZnSO4
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4. Aspects of Formation for Laity Both the Fathers of Vatican II and the bishops at the 1987 Synod on Laity use the word “integral” to describe the formation for laity. The lay apostolate can only be effective “through manifold and integral formation”. In discovering and living their proper vocation and mission‚ the laity must be formed according to the union which exists from their being members of the Church and citizens of human society. The many interrelated aspects of a totally integrated
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DETERMINATION OF ENTHALPY CHANGE OF NEUTRALIZATION IA Criteria Assessed: DCP CE MS Introduction When an alkali neutralizes an acid‚ a salt and water are formed. Aqueous hydrogen ions (H+(aq)) from the acid react with the hydroxide ions (OH- (aq)) from alkali‚ forming water. The identity of salt will depend on the nature of the acid and alkali used. H+(aq) + OH- (aq) → H2O(L) The combination of H+ and OH- ions in this way releases energy. In this practical‚ the enthalpy changes accompanying
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