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6. Check the results of the electrolysis. a) After you disconnect the battery, carefully mark the level of the water in each test-tube. b) Take out the test-tubes. Measure the difference between the start and end marks, to the nearest 0.1 cm. Fill in the table below. change in height (cm) volume of gas (cm3 = mL) H2 (cathode, negative terminal) Will be around 1 cm O2 (anode, positive terminal) Will be around 0.5 cm c) Measure the diameter of the test-tube, to the nearest 0.1 cm. Divide by 2 to get the radius. Radius of test tube = ____________________ cm d) In the table, fill in the volume of each gas using: V = pR2h e) Now compare to our predictions: Q10. Ratio of H2 to O2 gas: _____around 2:1______________ Part 2 – Industrial Application In this part you will see how industrial chemists use electrolysis to produce useful chemicals. 1. Mix up a different electrolyte solution by stirring together until fully dissolved: 3/2 cup water + 2 tsp table salt 2. Test apparatus using table salt electrolyte solution. a) Pour the saltwater solution into the cup with the pencils, and set up your electrolysis cell as before. Make a mark on each test-tube for the starting level of the water. Connect the battery. b) Set a timer for 5 min. At the end of this time, disconnect the battery. Meanwhile, go to step 3. 3. Table salt has the chemical formula NaCl. In water it breaks up into Na+ and Cl- ions. a) Atthecathode(negativebatteryterminal)youwillagainhavereduction,oradditionofelectrons to some chemical species. Q11. Balance the following possible reduction reactions: Using the table of reduction potentials, circle which reaction is actually going to occur. b) At the anode (positive battery terminal) there will be oxidation, or removal of electrons from Created by LABScI at Stanford 6PDF Image | Electrolysis splitting water
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