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Q29. What do you expect to be oxidized at the anode (positive battery terminal)? (i) H2O (ii) SO42- (iii) Cu(s) Q30. Write down the balanced chemical equation for the oxidation reaction: Q31. Do you expect to see bubbles at the positive terminal, negative terminal, both or neither? We expect to see bubbles only at the negative terminal, where hydrogen gas is still being formed. At the positive terminal, copper will be oxidized instead of water, so no gas is formed c) Hook up the other ends of the alligator clips to the terminals of the 9V battery. Let the reaction run for 3-5 minutes. Q32. Do you see bubbles at the electrode(s) where you expected to find them? Yes Q33. Why is it important that the pennies not be touching? If they are touching, the current will flow straight between the metal pennies and not through the solution at all. You will not see any chemical reaction, and you could easily short out the battery because pennies conduct electricity very well. Q34. Do you see any color change in the solution? The solution will likely turn some shade of yellow or light blue 4. When copper metal is oxidized, it can form both Cu+ and Cu2+ ions. Cu2+ ions are light blue. Cu+ can react with oxygen to form a yellow compound (Cu2O). Q35. Did your oxidation reaction produce Cu+, Cu2+ or a combination of the two? Either or a combination is possible Q36. When industrial chemists want to make chlorine and lye through electrolysis, why can't they not use electrodes made of common metals, such as silver or iron or zinc? These metals are more easily oxidized than chlorine (they lose electrons more readily), so metal ions will be formed instead of chlorine gas. 1C u ( s ) → 1C u 2 + ( a q ) + 2 e − Created by LABScI at Stanford 10PDF Image | Electrolysis splitting water
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