AM = atomic mass. valence is 2+
coulombs = amperes x seconds = 0.900 A x 60 min/hr x 60 s/min = 3,240 C.
96,485 C will deposit AM/2 grams of the metal
AM/2 x (3,240/96,485) = 3.368 g
Solve for AM. This looks like Hg to me and it's being phased out in batteries because of the environmental impact of Hg.
You conduct an experiment where you use a single battery with a charge capacity of 900 mAh to precipitate an unknown metal from a salt solution that was leaking from an old battery. You use a vast excess of the salt, so the amount of metal condensed is limited by the battery. You obtain 3.368 g of the metal. You can assume that the metal was the only substance being reduced in the electrochemical cell and 100% of the listed battery charge is useable. If you were able to determine that the metal ion was a +2 ion, then which metal is it? This metal was used in batteries for a long time (even in “alkaline” batteries) due to its good electrochemical properties, but it is now being phased out. Why? (Show your work for full credit) PLS HELP
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