Answer to Question #178642 in General Chemistry for Arsen

Question

A chemist reacted 17.25 grams of sodium metal with an excess amount of chlorine gas. The chemical reaction that occurred is shown.

__Na + __ Cl₂ → __ NaCl

If the percentage yield of the reaction is 88%, what is the actual yield? Show your work, including the use of stoichiometric calculations and conversion factors. 

Answer 1

Given,

% yield =$\dfrac{\text{ Reacted Na }}{\text{ Required Na}}\times 10$

$88=\dfrac{17.25}{\text{ Required (Na)}}\times 100$

$\text{ Required Na}=\dfrac{1725}{88}=19.60g$

Actual yield = $\dfrac{\text{ Reacted Na }}{\text{ Required Na}}\times 100$

$=\dfrac{17.25}{19.60}\times 100=88$ %