![]() ![]() A red litmus is inserted into the solution surrounding the electrode and it quickly turns blue.ī) Write the equation for the reaction occurring at this electrode.Ĥ) Name the oxidant and reductant taking part in the half reactions?ĥ) Write the equation for the overall reaction. View the video on the left and answer the questions below.ġ) What are the possible reactants present?Ģ) A brown substance is seen to form on the electrode on the leftī) Write an equation for the reaction that is occurring at this electrodeģ) A gas is seen forming on the electrode on the right. The power supply was then turned on and charge was allowed to flow for several seconds. The metal and hydrogen always forms at the cathode. A cotton wool plug was inserted at the bottom of the u-tube, as shown on the left. All ionic compounds when molten can be decomposed when electricity is passed through using electrolysis. Potassium iodide was placed in a u-tube and electrodes, attached to a power source, were inserted at each end. SolutionĮ) Which electrode would increase in mass? Explainį) Would a solution of PbBr 2 produce the same products? Explain using the table of half cell potential. Using a table of the electrochemical series answer the following questions.Ĭ) What type of reaction takes place at the anode and the cathode?ĭ) Write the equation of the reaction taking place at the cathode and the anode. ![]() The reaction proceeds when the switch is closed. ![]() The decomposition of molten lead bromide takes place using the apparatus shown on the right, where a current is passed through the electrodes. What reaction is occurring at the cathode? Why is NaCl electrolysed in the molten form to produce sodium metal as opposed to the aqueous form? The video on the right shows the electrolysis of a brine solution which is another word for concentrated NaCl solution. Step 2 Using the electrochemical series identify the strongest reductant that makes contact with the anode(+) or is the anode(+). Step 1 Using the electrochemical series identify the strongest oxidant that makes contact with the cathode(-) or is the cathode(-). So when predicting the products that will form at each electrode follow the two steps below Only when these have expired will the next strongest species, according to the electrochemical series react. The strongest reductant will be oxidised at the (+) anode and the strongest oxidant will be reduced at the (-) cathode. In an electrolytic cell the strongest oxidant and strongest reductant will react. The combination of electrocatalytic anodic oxidation with cathodic reduction can not only maximize the return of energy investment, but also produces value-added materials on both sides. Production of sodium takes place in industry in a special electrolytic An anode is an electrode of a device through which conventional current (positive charge) flows into the device from an external circuit, while a cathode is an electrode through which conventional current flows out of the device. To make efficient use of electrical energy in the whole electrocatalysis conversion process, the integrating of anode and cathode reactions plays a vital role. To form sodium metal with chlorine as a by-product. ![]() The sodium ions are attracted to the negative electrode (cathode) and To the positive electrode (anode) and undergo oxidation. Out of the anode and pumping them into the cathode. The power source simply acts as an electron pump pulling electrons Simple electrolytic process since only one reaction is possible at eachĮlectrode. Oxide ions react with oxidized carbon at the anode, producing CO 2(g).Of molten NaCl(pictured above) as our first example, as this is a relatively ![]()
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