Asked by hayley
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
Answers
Answered by
DrBob222
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.
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.