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

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Answer 1 · 2017-03-26T18:13:11

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

$64*g$ 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, ( $15.999*g*mol^-1$ ).

How much sulfate dianion, SO_4^(2-)SO_4^(2-) could be made from a 64*g64*g mass of dioxygen?