use electrochemistry to extract metals from ionic compounds in solution Procedure: -Start by attaching battery snap connector to a battery and fill beaker with 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
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g Mass of beaker with hydrated copper (II) sulfate 58.13 g Mass of hydrated copper (II) sulfate 3.02 g Mass of beaker with dehydrated copper (II) sulfate (last weighing) 57.22 g Mass of dehydrated copper (II) sulfate 2.18 g Mass of dehydrated copper (II) sulfate (2nd weighing) 2.11 g Questions 1. Calculate the value of “n”. Show your work. Include an example of ALL calculations involving solving for “n”. 3.02 g of hydrated copper sulfate is heated to drive off water. The dry sample
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oxygen gas‚ the rate of enzyme activity can be measured as the height of the column of oxygen gas bubbles produced in a test tube. If copper sulfate inhibits the action of catalase‚ then it will slow down the reaction between the catalase enzyme in chicken liver and hydrogen peroxide. The independent variable in this lab is the addition of copper sulfate to one test tube and the dependent variable is the amount of oxygen gas produced (measured as the height of gas bubbles). Procedure: Must include:
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products that are insoluble in water. In the three of the four reactions a cloudy white or yellow formed. This indicated the formation of a precipitate‚ caused by the generally insoluble phosphate anion. Potassium chloride‚ Iron nitrate‚ and potassium sulfate where the products which were soluble in water. With these products there was no evidence of a precipitate forming. 2. Based on the results from reactions A and B for the first group of reactions‚ the generally insoluble anion is phosphate. In
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noticed that a yellowish brown gas emerged‚ along with effervescence. The red solid disappeared and became a blue liquid. We know that we produced copper nitrate‚ nitrate gas‚ and water because the only two blue solutions in “A New Language” are copper sulfate and copper nitrate. It would make sense for us to have created copper nitrate‚ since we mixed copper with nitric acid‚ not sulfuric acid. The nitrate that we created was the brownish gas that we watched float up during the reaction. In addition‚ the
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majority of the Earth’s sulfur is stored underground in rocks and minerals‚ including as sulfate salts buried deep within ocean sediments. The sulfur cycle contains both atmospheric and terrestrial processes. Within the terrestrial portion‚ the cycle begins with the weathering of rocks‚ releasing the stored sulfur. The sulfur then comes into contact with air where it is converted into sulfate (SO4). The sulfate is taken up by plants and microorganisms and is converted into organic forms; animals then
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Reactions Purpose: To observe and differentiate between the four different types of chemical reactions. Variables: The independent variables are the sodium chloride‚ sodium carbonate‚ magnesium‚copper‚ copper (11) sulfate‚ silver nitrate‚ oxygen‚ lead(11) nitrate‚ sodium carbonate‚ copper (11) sulfate pentahydrate. The dependent variables are the chemical reactions that are being looked for. For example decomposition‚ synthesis‚ single displacement or double displacement of compounds or elements . Hypothesis:
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Copper-Iron Stoichiometry Lab Report 10/3/12 Abstract: The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate‚ CuSO4‚ mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was
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water. Therefore‚ Water of crystallization is water that is stoichiometrically bound into a crystal. Crystal salts containing water of crystallization are called hydrates. * Eg. CuSO4·5H2O cyrstals (copper(II) sulfate pentahydrate) Hypothesis In the hydrate copper (II) sulfate one mole of salt is believed to be combined with five moles of water. Bearing this in mind the following hypothesis was made: If the hydrate is heated until there is no further loss in weight‚ five moles of water will
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Discussion: For this experiment to occur‚ the limiting and the excess reagents needed to be determined. The limiting reagent was picked based upon the single displacement that was going to occur when the two substances‚ iron and copper(II)sulfate‚ were mixed together in water. Seeing that iron was going to displace copper and take its place‚ it was chosen to be the limiting reagent with the condition that if it was in excess then after the displacement was completed‚ there will be iron precipitate
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