Construction of a voltaic cell Consider a cobalt-silver voltaic cell that is constructed such that one half-cell consists of the
cobalt, CoCo, electrode immersed in a Co(NO3)3Co(NO3)3 solution, and the other half-cell consists of the silver, AgAg, electrode immersed in a AgNO3AgNO3 solution. The two electrodes are connected by a copper wire. The CoCo electrode acts as the anode, and the AgAg electrode acts as the cathode. To maintain electric neutrality, you add a KNO3KNO3 salt bridge separating the two half-cells. The half-cell is a chamber in the voltaic cell where one half-cell is the site of the oxidation reaction and the other half-cell is the site of the reduction reaction. Type the half-cell reaction that takes place at the anode for the cobalt-silver voltaic cell. Indicate the physical states of atoms and ions using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively.
A voltaic cell produces energy by spontaneous chemical processes. A voltaic cell contains an anode and a cathode. Oxidation (electron loss) occurs at the anode while reduction (electron gain) occurs at the cathode.
For the cobalt-silver voltaic cell, the reaction equation of the cobalt and silver voltaic anode half cell is shown;
At the anode;
Co(s) ------> Co^3+(aq) + 3e
Note that the anode is the electrode where oxidation occurs hence electrons are lost at the anode.
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Reason: The attraction between hydrogen and the electronegative atoms form the polar covalent bond. This bond can result in partial charges and attraction of molecules with opposite partial charges.
Working in laboratory is very dangerous when working with chemicals. It can burn the skin if it falls or if someone comes in contact with it. We should always be alert and be careful while handling chemicals in the laboratory. Safety measure should always be followed like wearing gloves and aprons. While mixing chemicals, always hold the flasks straight right in front of you with the help of a crucible tong or a test tube holder and move straight.