Experiment 12 Calorimetry and Heat of Reactions ____________________________________________________________________________________________________________ PERFORMANCE GOALS: 1. To learn how to use of a calorimeter 2. To learn how to collect and manipulate data in the computer 3. To calculate the calorimeter constant 4. To use Hess’ Law to find the heat or formation of magnesium oxide CHEMICAL OVERVIEW: • Enthalphy: (ΔH) : when chemical or physical changes occur at a constant
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1. Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) ( NO2(g) + O2(g)‚ with (H( = -199 kJ/mol‚ (S( = -4.1 J/K·mol. Calculate the (G( for this reaction at 25(C. A. 1020 kJ/mol B. -1.22 ( 103 kJ/mol C. 2.00 ( 103 kJ/mol D. -1.42 ( 103 kJ/mol E. -198 kJ/mol 2. For the reaction H2(g) + S(s) ( H2S(g)‚ (H( = -20.2 kJ/mol and (S( = +43.1 J/K·mol. Which of these statements is true? A. The reaction is only spontaneous
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Introduction: On a daily‚ millions of food products are exchanged and bought around the globe. Every person trusts that the Nutrition and Drug Label rely the proper information so they can make healthy and wise decisions about the food entering their body. This is essential to people who suffer from diabetes or other serious health problems. For consumers with high blood pressure‚ the incorrect salt intake can be deadly. However‚ the Food and Drug Administration allows there to be a twenty percent
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calorimeter was standardized using benzoic acid and the average heat capacity of the bomb calorimeter was calculated to be 10.60.3205 kJ/K. From that‚ the These results show that heats of combustions of unknown substances can be determined via bomb calorimetry. Introduction The first law of thermodynamics states that energy is conserved.2 Using that law it can be said that the change in the internal energy of a system () depends on the heat added (q) to the system and the work (w) done by the system
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Experiment 1 Calorimetry Chem 17 Univerity of the Philippines Diliman Discussion All chemical reactions involve energy. By understanding the behavior and connection of energy flow within a chemical reaction‚ we can understand and manipulate them to our advantage. The most common form of energy observed during chemical reactions is heat. The reaction may absorb (endothermic) or release (exothermic) heat‚ depending on the reacting substances. Calorimetry is the process of measuring the heat flow
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Experiment 11 Calorimetry and Hess’s Law Purpose- To determine the change in enthalpy for four reactions using calorimetry and Hess’s Law Procedures: A. Calibration of the Calorimeter 1. Obtain two copper cylinders and a Styrofoam cup with lid from your lab instructor. Check out a digital thermometer display from the storeroom window. 2. Set up a hot water bath using a 600mL beaker‚ ring stand‚ and Bunsen burner. Weigh the two copper cylinders
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the science lab. In science‚ we would participate in a lab. One of my favorite labs was the owl pellet dissection. Owl pellets are owl throw up. In owl pellets you can find the bones of animals the owl consumed. In this lab we were to take out the bones we found in the pellet and construct the animal we found inside. Most people‚ like me‚ had a sort of rodent‚ but some people found birds in their pellet. Another one of my favorite things we did in science was the Sharpie tie dye lab in fifth grade
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The experiment was done twice in trial 1 and 2. First‚ in the first trial‚ the crucible with lid was measured on a balance and the mass of them was recorded in grams which is m of clean crucible = 22.89g . This was followed by weighing the crucible with 0.3 g of Magnesium on a balance. The total mass of mg with the crucible was recorded which was m total mass mg + Crucible = 23.19g. Then the magnesium was heated using a Bunsen burner‚ and we put the crucible with Mg on a clay triangle using tongs
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CALCULATIONS Determining the amount Limiting Reagent used. nlimiting reagent = Molarity x Volume or Mass / Molar Mass Example: Limiting reagent is 5mL of 1.0 M HCl nlimiting reagent = Molarity x Volume nlimiting reagent = (1.0 [mol/L]) x 0.005 [L]) = 0.005 mol Determining the qrxn and qcal. qrxn + qcal = 0 -qrxn = qcal qrxn = ΔHrxn x nlimiting reagent qcal = Ccal ΔT qrxn = - Ccal ΔT + mcsolid ΔT (note: only if there is a precipitate formed in the reaction)
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Data and Observations: Part I Table: Metal: | Aluminum | Zinc | Iron | Copper | Mass of metal: | 27.776 g | 41.664 g | 34.720 g | 41.664 g | Volume of water in the calorimeter: | 26.0 mL | 26.0 mL | 26.0 mL | 26.0 mL | Initial temperature of water in calorimeter: | 25.3 °C | 25.3 °C | 25.3 °C | 25.3 °C | Temperature of hot water and metal in hot water bath: | 100.5 °C | 100.5 °C | 100.5 °C | 100.5 °C | Final temperature reached in the calorimeter: | 38.9 °C | 34.8 °C | 34.2 °C | 34
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