How much sulfate dianion, #SO_4^(2-)# could be made from a #64*g# mass of dioxygen?

1 Answer
anor277
Mar 26, 2017

You mean #"sulfate ion"#, #SO_4^(2-)#.........

Explanation:

#64*g# of oxygen atoms represents #(64*g)/(16.0*g*mol^-1)# #O# #=# #"4 moles of oxygen atoms."#

And thus, with mole of sulfur atoms, i.e. #32*g#, we could make #96*g# sulfate dianion, i.e. #SO_4^(2-)#.

All we have done here is to take equivalent masses of sulfur (#32.06*g*mol#) and oxygen, (#15.999*g*mol^-1#).

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