Metal In Geolo Deposite In Electrode Purpose Electrochemistry Electrochemical Cells Overview In An Electrochemical 1 (58.87 KiB) Viewed 21 times
Metal In Geolo Deposite In Electrode Purpose Electrochemistry Electrochemical Cells Overview In An Electrochemical 2 (23.15 KiB) Viewed 21 times
METAL IN GEOLO DEPOSITE IN ELECTRODE . . PURPOSE . Electrochemistry Electrochemical Cells OVERVIEW In an electrochemical cell, chemical energy is converted into electrical energy. This accomplished by using a spontaneous chemical reaction to generate an electric current, which we can simply define here as electrons traveling though a wire. . . . To create the electrochemical cell two half-reactions will be set up in different containers. In one, an oxidation reaction will be used to generate a source of electrons. These free electron will travel, through an external circuit, to the second container and will cause the reduction reaction to occur. The final requirement for our complete electrochemical cell will be a salt bridge that will permitions to flow between the two half-cells, thus maintaining electrically neutral solutions. . SAFETY elect Zna)-Zn(aq) +20 Anode IONS EQUIPMENT AND MATERIALS o(+20) Code reduction To build several electrochemical cells. Follow normal lab safety guidelines. There are no specific safety hazards for this lab. 250-ml, beakers, 2 glass U-tube for the salt bridge cotton plugs for the salt bridge copper wires, 2, insalated, with alligator clips steel wool to clean electrodes DC voltmeter metal electrodes: copper, zinc, lead Electrochemistry Electrochemical Celle 6.5M CO 0.5M Zz NO 0.5MM ONO 6.SM KI 0₂-for the salt bridge PROCEDURI: 1. Each half-cell will be created by placing a metal electrode in an electroly a solution containing the metal's lows For care se the copper electrode will be placed in a copper) with te solution For ch elects chemical cell- two half-celle let the cells be connected U-tube 2. Fill a beaker at sot owo-dhids full of the electrolytic tion Cles the electrode using the steel wool, the place the elects xde in its appropriate solution. 1. Clip and each copper wire to the two electrodes wing the alligs or clips. Fill the U-tabe with NO, and stopper both ends with de com phags T n the U-abe upside down and place one end in each hal-cell 5. Teach the othe end of the copper wires to the voltmeter terminals. If the indicator on the voltmeter deflects in the wrong direction switch the wires on the terminals. Read the highest volt ge reading obtained-you'll need to do this quickly afr connecting the wires to the voltmeter. 6. Repeat the experiment for other combinations of half RESULTS will require other-they will Copy a data table imilar to the one shown below into your lab notebook and use it to record your results Half-ce is CujC₂² Zaza CalCu"&gMg ZaZa MgMg Voltage 193 100 .534 FRENO 24 Cu + Ze → Cu (3)| +0.34% (₁) ORIL E READ (CATION) - EREAD (ONOOE) Z₁² (aq) + 2 €¯ -> Z₁ (5) -0.76 V M₂² (aq) +22² Mg(s) -2.37 v
2. Using a Table of Standard Reduction Potentials, calculate the ti eoretical voltage for each cell. 3. Compare the voltages you obtained with the theoretical vol age for each cell. What are some reasons that w uld account for any differences?
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