Chemist carries out this reaction and obtains 11.4 g of tungsten. if the percent yield is 89.4%, The mass of WO₃ was used is 16.1 g.
given that :
percent yield = 89.4%
theoretical yield = 11.4 g
the percent yield = (actual yield / theoretical yield ) × 100 %
Theoretical yield = (actual yield / percent yield ) × 100 %
= (11.4 g / 89.4 ) × 100 %
= 12.8 g
The mass of the WO₃ = (12.8 g W / 183.84 g/mol W ) ×231.84 g/mol WO₃
= 16.1 g WO₃
The mass of was used is 16.1 g.
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