reactions work and what products they may form. Materials & Procedure Materials: * Wood Splints - Copper Sulfate * Sodium Sulfate - Copper Wire * Barium Chloride - 6% Hydrogen Peroxide * Mossy Zinc - Copper Sulfate Pentahydrate * Hydrochloric Acid - Iron Filings * Manganese Dioxide Procedure: Reaction A Place a scoop of copper (II) sulfate pentahydrate crystals in a clean‚ dry test tube. Use a test tube holder to position the test tube over a burner
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much heat is this in calories? Chapter 4 Identify X: Give the formula for the compound formed from the most common ions of Ca and O Chapter 5 Name the following compounds: P4O10 CoCl3 Li3P HClO3 RbOH Calculate the formula mass of copper(II) sulfate pentahydrate (CuSO4·5H2O) Chapter 6 Calculate the number of moles and number of molecules in 65.78 g of H2O. How many H atoms and how many O atoms are contained in this sample? NutraSweet is 57.14% C by mass‚ 6.16% H by mass‚ 9.52% N by
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limiting reactant of a chemical reaction that involves iron filings and a copper sulfate solution. Second‚ to determine the mole ratios between iron and copper and to show that a single replacement reaction occurs when iron and copper sulfate react with each other. And lastly‚ to determine/calculate the percent yield to better analyze the chemical reaction between iron and copper sulfate to produce copper and iron sulfate. The method used to perform this lab will be to combine a metal with a solution
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other objectives of the lab which are learning what are concentrated‚ diluted‚ supersaturated‚ and saturated substances and how can they be identified. The hypothesis of this lab would be that when temperature increases‚ the amount of salt and copper sulfate that can be added in the water and be dissolved will increase. Theory: The hypothesis will be proven because when temperature is increased‚ energy is released and this energy breaks the forces that held up the atoms together of a substance
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hydrate of copper (II) sulfate hydrate. Hypothesis: I hypothesize that when the solution is heated the hydrate will convert to an anhydrous ionic compound. Then the percentage composition will be determined by weighing the mass of the white crystals. Materials: 400ml beaker‚ hot plate‚ tongs‚ scoopula‚ electronic balance‚ glass rod‚ hot pad‚ and 4g of hydrated copper (II) sulfate Procedure: 1. Measure the mass of the beaker and stirring rod. 2. Add 4g hydrated copper (II) sulfate to the
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605g)*100=76% | 100%-76%=24% | (0.990g/0.566g)*100=57% | 100%-57%=43% | Average Value of Salt in a Hydrate | (76%+57%)/2=66.5% | Average Value of Water in Hydrate | (24%+43%)/2=33.5% | Result of the lab was: The given hydrate is CuSO4 5H2O (Copper II Sulfate Pentahydrate) The calculated value percentage of the Salt in hydrate (66.5%) and Water in hydrate (33.5%)‚ suggests that the given initial compound is CuSO4
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used were copper sulfate (blue crystals)‚ sodium chloride (salt)‚ and iron. Copper sulfate is a chemical compound which is produced commercially by reacting various copper (II) compounds with sulfuric acid [1]. It generally appears as a bright blue or green crystal [1]. Its chemical formula is CuSo4. Iron is silver-white magnetic metallic and readily rusts in moist air [3]. Its chemical formula is Fe. The chemical reaction was demonstrated by the iron reacting to the copper sulfate.
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number of moles of anhydrous copper sulfate‚ percent comp of water in the hydrated copper sulfate‚ the mole ratio of moles of water and moles of anhydrous copper sulfate. Once this is all done‚ we found our percent error and compared it to the exact value. In the lab‚ we used the following tools: lab apron‚ lab goggles‚ clay triangle‚ bunsen burner‚ ring stand‚ flint striker‚ electronic weight‚ crucible‚ crucible tongs‚ scoopula‚ gas line‚ beaker‚ copper (II) sulfate‚ and paper towels. To begin
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between 100 and 200 mL of copper (II) sulfate solution -Connect clip to each of the nickel strips -Place nickel strips in copper sulfate solution without strips touching -Put one clip on the positive side of the battery and the second to the negative side. Observe -Switch clips to the opposite charged sides of the battery. Observe again -Reverse wiring to original spots Observations Q-what did you observe when you hooked up the nickel strips to the battery? A-the copper from the solution coated
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Enthalpy changes can be calculated using average bond enthalpy data. i) The enthalpy change to convert methane into gaseous atoms is shown below. [pic] Calculate the average bond enthalpy of a C—H bond in methane. [1] ii) Use the data in the table below and your answer to (a)(i) to calculate the enthalpy change for [pic] [3] [pic] b) The standard enthalpy of formation of 1‚2-dibromoethane‚ CH2BrCH2Br‚ is – 37.8 kJmol-1. Suggest the main reason for
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