In the Reactions with Copper experiment, why was it important to use as littlezinc as possible (just enough to complete the reaction) when reducing andforming the copper metal at the end of the lab?
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In the Reactions with Copper experiment, why was it important to use as little
zinc as possible (just enough to complete the reaction) when reducing and
forming the copper metal at the end of the lab?
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Solved in 2 steps
- Explain the importance of using copper and zinc plates in this experiment? Be as specific as possible (e.g. Redox reaction, oxidation half-reaction, reduction half-reaction, oxidizing agent, reducing agent).Solvent is purged with N₂ to remove O₂. What electrochemical process are we trying to eliminate by removing the oxygen?help me asap pls
- Please Help!! Part A: Electrochemical Cell Mass Data for Electochemical Cell Copper Zinc Initial mass of strip (g) 2.421 2.436 Final mass of strip (g) 2.602 2.250 Measured Ecell (V)= 1.02 Part B: Electroplating Mass Data for Electoplating Mass (g) Initial 0.930 After first plating 1.083 After second plating 1.238 After third plating 1.377 Part A: Electrochemical Cell Table view List view Mass Calculations for Electochemical Cell Copper Zinc Initial mass of strip (g) 2.421 2.436 Final mass of strip (g) 2.602 2.250 Mass gained(+) or lost(−) (g) 0.18 -0.19 what is Computed Ecell (V)? what is Computed ΔG (kJ/mol)? Mass Calculations for Electroplating (fill in chart) First Second Third Final mass of paper clip (g) 1.083 1.238 1.377 Initial mass of paper clip (g) 0.930 1.083 1.238…A calculation in Model 1 shows that an electrical current of 7.50 A deposits 4.56 g of Fe in 35.0 min. Using this calculation, answer: a) How many moles of electrons flowed through the cell in 35 minutes? b) How many moles of Fe were plated onto the cathode in 35 minutes? c) Why is the ratio (moles of electrons)/(moles of Fe)=2?which gas formed at each electrode in the electrolysis of water (the Petri dish where you did NOT add KI)? What experimental evidence indicates this? Explain your reasoning
- How many moles of Fe^2+ ion can be oxidized by 1.2 ×10^-2 moles MnO4 ion in the reaction between MnO4 ion and Fe^2+#4The aluminum sample is not cut into small pieces but rather left as one large piece. a. How will this oversight affect the progress of completing the experimental procedure? Explain. b. Will the percent yield of the alum be too high, too low, or unaffected by the oversight? Explain.
- Make an inference about the effect of applied current and electrolysis time on the mass of deposited copper. Thoroughly explain and relate any observed trend to Faraday’s Law of Electrolysis.a. What happened to the mass of deposited Cu when the applied current is increased, as shown in Setups 1 and 2? b. What happened to the mass of deposited Cu when the electrolysis time is increased, as shown in Setups 2 and 3?When the molecular reaction between sodium silicate and copper(II) nitrite is balanced correctly the stoichiometric coefficient for sodium nitrite is _____.Please help me