Posted by andrea on .
The following reaction is used to produce tungsten(VI)oxide: WS3(s) + O2(g) ¨ WO3(s) + SO2(g)
The WO3 is then heated and undergoes a decomposition reaction produce tungsten and oxygen gas. How many grams of tungsten could be produced if 39.27 grams of WS3 are used
You should first balance the equation given.
WS3(s) + O2(g) -> WO3(s) + SO2(g)
But you should see that one mole of WS3 must yield one mole of WO3.
You also have the decomposition of WO3
WO3 -> W + O2
Again one mole of WO3 yields one mole of W metal.
So calculate the number of moles of WS3 you are starting with from
39.27/(molar mass of WS3)
this is the same number of moles of W metal produced so mass produced
39.27x(molar mass of W)/(molar mass of WS3)