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Q5. Balance the following possible reduction reactions. There must be the same number of each atom on each side, and the total charge must be the same on each side. Look at the table of standard reduction potentials at the end of your lab. Which reaction is preferred? (i.e. is Mg2+ or H2O more easily reduced)? Circle the appropriate equation above. Water (H2O) is more easily reduced. Q6. What are the bubbles being formed at the cathode (the pencil connected to the negative terminal)? Hydrogen gas (H2) b) The positive terminal of the battery is connected to the anode. Electrons are pumped into this electrode. Once they reach the solution, they participate in an oxidation reaction – a chemical reaction where some chemical species loses electrons. In the Epsom Salt solution, there are two species that could be giving up electrons: the SO42- ions or the water molecules themselves. Q7. Balance the following possible oxidation reactions. Look at the table of standard reduction potentials at the end of your lab. Which reaction is preferred? (i.e. is SO42- or H2O more easily oxidized)? Circle the appropriate equation above. Water (H2O) is more easily oxidized Q8. What are the bubbles being formed at the anode (the pencil connected to the negative terminal)? Oxygen gas (O2) Q9. What would you expect for the ratio of how much gas is formed at the cathode to how much is formed at the anode? Hint: electrons are pumped into the cathode at the same rate as they are pumped out at the anode, so look at the relative number of electrons in your circled reactions. ___2____ units of gas at the cathode : ___1___ units of gas at the anode From the balanced equations, making one molecule of H2 at the cathode requires 2 electrons and making one molecule of O2 at the anode gives off 4 electrons. That means that for every 4 electrons that go through the circuit, we get 2 moles of H2 and one mole of O2 – a 2:1 ratio Created by LABScI at Stanford 5PDF Image | Electrolysis splitting water
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