Solution:
The process is carried out in an electrolytic cell, which consists of two electrodes an anode and a cathode with an external electrical energy supply. The impurity in copper oxide decreases the solubility, and therefore decreases the rate of reaction in electrolytic cell because precipitation usually occurs in a solution that is rich in dissolved solids. Therefore, process requires longer time in impure sample.
Why does an electrogravimetric determination of copper in an impure sample of copper oxide take so...
Electrogravimetric determination of Copper: 1. Why the sample solution is blue colored? Why do the electrodes have to be as close as possible? 2. Using your textbook explain why does the experiment take so long? 3. Identify three factors that influence the physical characteristics of an electrolytic deposit. 4. What where the acids used in the acidic digestion? Why the experiment requires a mixture of acids? rather than a single one? 5. Why is important to avoid mixing acetone with...
The Purification of copper can be achieved by electrorefining copper from an impure copper anode onto a pure copper cathode in an electrolytic cell. How many hours will it take to plate 16.5 kg of copper onto the cathode if the current passed through the cell is held constant at 35.0 amperes? Assume the copper in the electrolytic solution is present as Cu2+. (Faraday’s Constant = 96500 Coulombs/mol e–).
write clearly d. 0.626 g sample of copper oxide was reduced to 0.500 g of copper metal by heating in a stream of hydrogen. Calculate the empirical formula of the copper oxide sample. 2 marks
Given the following data, calculate the mass percentage of copper in the unknown copper oxide sample for this particular trial. Mass of empty test tube: 2.319g Mass of test tube and unknown copper oxide sample: 2.943g Mass of test tube and product (after reaction): 2.630g
Explain why the melting point depresses and broadens when a sample is impure .
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A 10g sample of lead and a 10g sample of copper are both heated so that their temperatures increase by 10°C. Did both metals absorb the same amount of energy to do this? Explain why or why not. (2 marks)
When sulfuric acid and copper (II) oxide are allowed to react, copper (II) sulfate is formed. Why did you wash the precipitated copper oxide with water? What observation might you make that suggests that a chemical reaction has occurred?
In the Idometric Analysis of Copper Oxide, why did I not need to accurately weigh out the KI used in the standard and unknown analysis?
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