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
- Give the balance reaction of the given compound in the experiment and also give the two half reactionsHow many electrons have been gained by vanadium in the given half reaction?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).
- 2. 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 increasedb. What happened to the mass of deposited Cu when the electrolysis time is increasedHello I need help with the following questions. I will also attach a picture of the questions with the graph. Post-Lab Questions The oxidation-reduction reaction that was performed in this experiment is: Why does this oxidation result in a color change? What color change did you observe? Why do you think the temperature of the reaction increased as the reaction proceeded? Use scientific reasoning in your explanation. How would the reaction change if you added 2 g of steel wool to the acetate and reduced the iron acetate solution down to 50 mL (evaporated off 100 mL)?Why do you need to clean the electrodes before you start the experiment? Why is it important that the electrodes do not touch each other inside the lemon?
- 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?Write out the half reaction as it would actuall Accur at the anode. And is there a min or a max standard reduction.
- Write the overall reaction that occurs during use (discharging) of nickel-cadmium cell. Is it a primary or a secondary cell? Mention its one merit over the lead storage cell.Match each phrase with its correct term. Record your responses onto the Google Form. 13. -log [H,O'] 14. 6.022 x 10 units/mol 15. The unit of measure for concentration. 16. Where reduction takes place in a galvanic cell. 17. Balances the change in positivity and negativity of galvanic cell solutions. 18. The oxidation state of pure elements. 19. The electrostatic attraction between oppositely-charged ions. 20. Organic compounds containing the maximum number of hydrogens possible. a. salt bridge b. cathode с. рH d. zero e. hydroxyl f. Avogadro's number g. saturated h. mol/L i. ionic bondMake 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?