Introduction The first law of thermodynamics states that the energy of the universe is constant. Heat is transferred when the atoms of one material vibrate and collide with the atoms of another material‚ thus transferring energy. For this reason‚ heats always travel from hot to cold objects and two objects will reach an equilibrium temperature. Materials and Methods 1. Oven 7. Test Tube 2. Pasco Temperature Probe 8. Stopper 3. Scale 9. Calorimeter 4. Samples of Metals
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Post lab The unknown solution 4055 was tested by the separation scheme in order to identify the four cations that exist in it. The cations found were Ag+‚ Ba2+‚ Mn2+‚ and Ni2+. When I added 5 drops of 3M NaCl to the unknown solution‚ we had some precipitate‚ we centrifuge and then we divided to two test tubes‚ and they were put in hot water and got confirmatory tested. The Ag+ appeared to be in the solution because it melted‚ however Pb2+ didn’t. With the rest of the solution we added Na2SO4 we had
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1 Weigh the beaker. 2 Add 50 milliliters of the solution you want to test to the beaker and record its mass. The mass of the solution is equal to the total mass minus the mass of the beaker. 3 Divide the mass of the solution by its volume -- in this case‚ 50 milliliters -- to find its density. 4 Empty‚ rinse and dry the beaker. Add 4.3 grams of sugar to the empty beaker‚ then add water until the contents reach 50 milliliters in volume. Stir until the sugar dissolves‚ then measure the
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I. Objective: The objective of this experiment is to determine the mass percent of iron in an iron compound using a spectrophotometer. From there‚ determine which iron compounds are in the stock room bottles based off of the experimental mass percent results. II. Introduction: The objective is to determine the mass percent of iron in an iron compound using a spectrophotometer. From there‚ determine which iron compounds are in the stock room bottles based off of the experimental mass percent results
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First‚ prepare a data table. Record what you see throughout the laboratory activity. Your teacher will demonstrate for the class the reaction of metallic copper with concentrated nitric acid‚ HNO3. This must be done in the fume hood. (Caution: Avoid breathing poisonous gases. Avoid contact of skin with nitric acid. It burns skin and clothing.) One student will be asked to feel the side of the demonstration beaker and report to the group. The products formed are copper(II) nitrate solution‚ Cu(NO3)2(aq)
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MODULE 2 WORKSHEET 6 CALCULATIONS INVOLVING GASES Syllabus reference 9.3.2 1 Two identical gas flasks‚ A and B‚ are kept at the same temperature and pressure. Flask A contains 10 g of ethane gas‚ C2H6. Flask B contains sulfur dioxide gas‚ SO2. Calculate the mass of sulfur dioxide gas in flask B. moles ethane 10/30 0.33 mol moles SO2 0.33 mol mass SO2 0.33 64 21 g 2 What mass of nitric oxide‚ NO‚ is present in a 2.5 L flask at a pressure of 100 kPa and 0ºC? mole NO 2.5/22.71
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Class average for a 80 and 120 drop count was recorded to be 0.041+/- 0.005 mL/drop. If a graduated cylinder is not available there is another way of adding more of the solution. The disposable pipet can transfer 0.5mL of the solution to the chemical reaction. When comparing a 10mL graduated cylinder‚ a 100mL beaker‚ and a 50mL graduated cylinder‚ the most precision peace of glass wear would be the 10 mL graduated cylinder with the true volume of water (calculated)‚ class average‚ and uncertainties
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Experiment 3: Separating and Determining the Mass of Calcium Ion in a Calcium-Enriched Tablet In this lab‚ we dissolved a calcium-enriched tablet and participate the calcium ion as calcium carbonate. Our purpose is to determine the masses of calcium carbonate and calcium ion‚ to determine the mass percent of calcium ion in the tablet and to compare the masses and the percent with the listed tablet ingredients. This time we used a 150mL beaker‚ analytical balance‚ forceps‚ a 50mL graduated cylinder
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In the first process of the lab‚ you measure the mass of water transferred from a buret to a beaker‚ to determine the experimental mass of the water‚ and the volume of the water collected. We measured the temperature of the water so we could calculate the density of the water‚ which enabled us to calculate the actual volume of water‚ by using the density and the measured volume of water. To determine the percent error‚ we had to subtract the actual volume of water by the experimental volume of water
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One of the wonders of this planet is water. Water makes up 65% of humans‚ and 70% of the Earth. It is also common knowledge that humans cannot survive three days without it. Water is essential. If almost three-fourths of Earth is made up of water‚ why are there still so many people in the world suffering from a lack of it? Although not all water can be used for drinking purposes‚ in many places‚ water that is drinkable- is polluted or deluded by many agricultural and industrial motives and damage
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