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).Fill in the coefficients you get from balancing the the reaction below using the half-reaction method. Be sure you simplify all the coefficients into the smallest whole number ratios for this fınal answer (i.e.- Standard Form). If the substance does not appear in the final equation put a "0" for the coefficient and don't forget to place a "1" in the spaces where the coefficient of 1 goes. If you leave the space blank it will be marked incorrect. (Reaction j) MnO4 (aq) + CH5CH3(aq) + H20(1) + H*(aq) ----------> C6H&CO2(aq) + Mn2 (aq) + H2O(1) + H*(aq) How many electrons were transferred in the balanced reaction? electronsSolvent is purged with N₂ to remove O₂. What electrochemical process are we trying to eliminate by removing the oxygen?
- Curriculum Expectation. investigate oxidation-reduction reactions using a galvanic cell, and analyse electrochemical reactions in qualitative and quantitative terms;help me asap plsPlease 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…
- #2A 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?please answer
- 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+31. In the reaction: Cr2O72- + 6S2O32- + 14H+ → 2Cr3+ + 3S4O62- + 7H2O, S2+ is being reduced. True FalseUse the mole of electrons is 0.00314 and the half the reaction for the anode to calculate the predicted mole of Cu oxidized at the anode.