You conduct an experiment where you use a single battery with a charge capacity
ID: 963014 • Letter: Y
Question
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?
Explanation / Answer
W=MIT/ZF Z=+2 F=96500 M=molecular mass from which we have to identify the element
W=weight of metal I=current T=time
so M=3.368*2*96500/0.9*3600=200.62 g
it is the mass of
Due to the content of toxic mercury and environmental concerns about its disposal, the sale of mercury batteries is now banned in many countries
Hg Mercury