This problem is providing us with the reaction whereby tungsten is produced from tungsten (VI) oxide and hydrogen, so the percentage atom economy is required and found to be 64.3 % according to:
In the ambit of green chemistry, atom economy is one of the twelve principles of green chemistry, and tell us how efficient a chemical process is, in terms of the necessary reactants, versus the yielded products. In the ideal case, it is 100 % meaning that all the reactants lead to the desired product.
However, when byproducts are present, this percentage dwindles and the idea is to reason how convenient the process is. In this case, we can calculate the atom economy, by simply dividing the atomic mass of tungsten by the addition of the molar mass of tungsten (VI) oxide and three times that of waters:
[tex]\%A-E=\frac{183.84g/mol}{231.84g/mol+3*18.02g/mol} *100\%\\\\\%A-E=64.3\%[/tex]
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