measuring enthalpy changes In all the following questions‚ assume that the densities and specific heat capacities of the solutions are the same as pure water i.e. ρ = 1.0 gcm-3 and c = 4.18 Jg-1K-1 1. Zinc will displace copper from copper (II) sulphate solution according to the following equation: CuSO4(aq) + Zn(s) ( Cu(s) + ZnSO4(aq) If an excess of zinc powder is added to 50 cm3 of 1.0 moldm-3 copper(II) sulphate‚ the temperature increases by 6.3 oC. Calculate the enthalpy change
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Christina Park 2/14/12 pd.3 Chapter 11 Notes I. Measuring Matter A. Counting Particles number of unit for counting is always constant. a. What is a mole? mole (mol): the SI unit used to measure the amount of a substance‚ number of representative particles. representative particle: any kind of particle such as atoms‚ molecules‚ formula units‚ electrons‚ or ions. Avogadro’s number: 6.022 136 7 x 10²³‚ volume of one mole of a gas determined by Amedeo Avagadro in 1811. B. Converting
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mL) Safety goggles Lab apron Plastic gloves Full face shield Reagents Zinc Magnesium Iron Copper 1M hydrochloric acid‚ HCl 1M sulphuric acid‚ H2SO4 1M acetic acid‚ HC2H3O2 1M phosphoric acid‚ H3PO4 Procedure: Please refer to Health Chemistry‚ Laboratory Experiments‚ page(s) 75-76. Data and Observations: Table 1: Comparison of Metal Activities Zinc Magnesium Copper Iron Hydrochloric acid Small bubbles Many bubbles N.R. color change (black) Sulfuric acid
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Compound Katie Sanders Science Block 3 February 29‚ 2012 Title: Analysis of a Hydrated Crystalline Compound Purpose: The purpose of our experiment was to determine the amount of water in copper sulfate pentahydrate expressed as a percent. Hypothesis: I think that bluestone crystals are 20% water‚ because it’s called pentahydrate (penta means five) and 1/5 of 100 (since it’s expressed as a percent) is 20‚ so I think bluestone crystals are
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cylinder {± 0.5cm³} • Different chemicals Introduction/Theory: Exothermic reactions are those reactions that release energy in the form of heat. Endothermic reactions need to absorb energy in the form of heat to proceed. Enthalpy is the heat content of a substance. Enthalpy change is positive for an endothermic reaction‚ as energy is absorbed {for example in the form of heat absorbed‚ the test-tube becomes cool to touch} and negative in the case of exothermic reactions {the test-tube becomes warm/hot
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lowest out of the 3 trials at 1.68 volts‚ thus proving that the higher concentration the lower the voltage. When the concentration of the product decreases‚ it will drive the equilibrium to the right to minimize the impact. Although‚ the lowest calculation (0.5 mol dm-3) is not necessarily the highest out of all 3 trials‚ it is not far off from 1 molar solution‚ only 0.2 Volts. The system’s attempt to remain at equilibrium by minimizing the impact‚ refers to le Châtelier’s Principle. The voltage is
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reaction. Copper(II) oxide will be synthesized from a known mass of copper(II) sulfate pentahydrate. Using the relationship of the balanced equation‚ and other stoichiometry relationships‚ you will calculate a theoretical yield of CuO‚ and your actual yield. You then will calculate a percent yield. Copper(II) sulfate pentahydrate will be dissolved in water and reacted using a double replacement reaction with sodium hydroxide. The addition of hydroxide ions to a solution containing copper(II) ions
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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 to the nearest 0.01 grams. Carefully place the two copper cylinders in a 25mL test tube. Place
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by the molar mass. Experiment 1 First I took a crucible‚ a balance‚ and a Bunsen burner and placed them onto the workbench. Then I measured the mass of the empty crucible with the balance and recorded it in my notes. Next I added 5 g of the copper sulfate hydrate to the crucible. I measured the mass of the crucible with the balance and recorded it in my notes. Then I moved the crucible onto the Bunsen burner and
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anhydrous salt. 8. Pour and scrape the anhydrous salt into trash‚ and clean up. Make sure to wash crucible with soap. Results & Calculations Data: Mass of empty crucible: 32.67 grams Mass of crucible and hydrate: 34.1 grams Mass of crucible and anhydrous salt: trial 1 (33.93g); trial 2 (33.51); trial 3 (33.51) Mass of water: 0.59g Mass of anhydrous salt: 0.84g Calculations: Water: 0.59g/18=0.033; 0.033/0.00526= 6.27 Anhydrous Salt: 0.84/159.61= 0.00526; 0.00526/0.00526=1 Coefficient of H20: 6 Percent
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