Data collection and processing Qualitative observation Before * Blue solution of copper sulfate * Grey zinc powder During * Blue color solution changes to greyish black * Heat is given out‚ so the surroundings become hotter. After * Grey powder remains on the sides of the cup * Precipitate formed at the bottom of the cup List of chemicals and apparatus used Chemicals used Copper sulfate solution‚ 1 mol dm-3 25g of zinc powder Apparatus needed
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time‚ the enthalpy change of the reaction can be experimentally determined. Assumption 1. Mass of H2O in 100cm3 of CuSO4 solution is 100g 2. Specific heat of solution is 4.18 kJ kg-1 K-1 which is the same as the specific heat of water 3. Heat evolved in the reaction will be absorbed by the CuSO4 solution 4. Maximum temperature that would have been reacted if no heat lost to surroundings can be calculated by extrapolation the graph plotted with temperature against time. Procedure
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be copper (II) sulfate pentahydrate – CuSO4·5H2O. I. INTRODUCTION Hydrates are chemical compounds that contain discrete water molecules as part of their crystalline structure. Water is bound in most hydrates in definite‚ stoichiometric proportions‚ and the number of water molecules bound per metal ion is often characteristic of a particular metal ion. Many hydrated salts can be transformed to the anhydrous (without water) compound by application of heat. In this experiment‚ we determine the
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compounds or elements . Hypothesis: Part 1 : I believe that magnesium burning in oxygen will have synthesis reaction because the magnesium will react with the oxygen in the air forming MGO where before the two elements were separate but with added heat they have been able to become a new compound. Part 2: I believe that when the sodium chloride and silver nitrate are mixed a double displacement reaction will occur‚ making sodium nitrate and silver chloride because sodium is very reactive and therefore
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crystals in a clean‚ dry test tube. Use a test tube holder to position the test tube over a burner flame. Heat until no further change is observed. Allow dehydrated crystals to cool and add 5 drops of water. Reaction B Place 1 squirt of sodium sulfate in a test tube. Add a squirt of barium chloride solution. Reaction C Using crucible tongs‚ heat a 5 cm piece of copper wire to red heat for 30 seconds in the hottest part of the burner flamer. After the wire cools‚ scrape its surface with the
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HOW TO USE A SCIENTIFIC CALCULATOR How to use a Scientific Calculator: entering expression‚ angle measure‚ number formats‚ arithmetic operators‚ positive numbers‚ negative numbers‚ scientific notation‚ parentheses‚ chemical formulae‚ physical constants. Entering expression Type your expression directly onto the input line or copy and paste an expression from another programs. When you finish entering your expression‚ pres ENTER or click [=] button. Spaces are irrelevant‚ for example 54 + 3*2
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The Dehydration of a Bluestone February.28.2008 Purpose • To determine the value of X in CuSO4 • xH2O. Materials • Crucible • Blue Stone • Bunsen Burner • Bunsen Lighter • Test Tube • Water • Rheostat • Clay Triangle • Electronic Balance Procedure A clean crucible was taken and weighed on an electronic balance. The mass was then written down. 2g of bluestone was placed in the crucible and weighed. The mass of the blue solid was written down. The crucible was placed on a clay
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empirical formula of the hydrate and its percentage by mass of water. Hypothesis: If the hydrated form of CuSO4 is heated then it will remove the water turning it to the anhydrous form then it will change from blue to white. Materials: * Balance * Crucible and Cover * Crucible and tongs * Distilled water * Spatula * Stirring rod‚ glass * Bunsen burner * CuSO4‚ hydrate crystals * Desiccator gauze * Dropper or micropet * Ring Stand * Ring and pipe-stem
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Before we heated the blue CuSo4 Solution‚ there were still some crystals remain in the bottom. But when we finished heat the solution‚ the crystals were completely dissolved. (CuSo4 solution was blue) While we added 1.49 gram of iron filings (black) in to the breaker in small increments. But there were some Iron filings left on the weight cup. In the first
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After this lab‚ I learned that the water in CuSO4* 5H2O can be removed by heating it with a propane burner. After the water was evaporated‚ you can use the loss in mass to calculate the amount of water initally in copper (II) sulfate pentahydrate. Once all water in copper (II) Sulfate pentahydrate
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