Answer to Question #267085 in General Chemistry for jho

Question

1. Tungsten carbide (WC), used in making tools and jewelries, is produced by the reaction of tungsten hexachloride (WCl6), H2 and CH4 at 670℃.

WCl6 + H2 + CH4 WC + 6HCl

If 23.5 g WCl6 reacts with excess H2 and CH4, and 10.8 g WC are recovered, what is the percent yield?

Answer 1

Taking W=183.84 Cl=35.453 C=12.0107

WCl₆= 183.84+ (35.453×6)= 396.558g

WC= 183.84+ 12.0107

= 195.8507g

396.558 of WCl₆ yields 195.8507 of WCl₆

23.5g of WCl₆ in the same proportion should yield

$=\frac{23.5}{396.558}×195.8507=11.6061g$

of WCl₆

Actual yield given = 10.8g

$\%$ yield $=\frac{Actual \>yield}{Theoretical \> value}×100\%$

$=\frac{10.8}{11.6061}×100\%=93.06\%$