PLEASE HURRY. I'LL MARK BRAINLIEST!! 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.

Explanation:

Step 1

Amount of Na metal = 17.25 grams

Percentage yield of reaction = 88%  

Actual yield = ?  

Step 2

The balance chemical equation :

2Na(s) + Cl2(g) > 2NaCl(aq)  

We know that -

Molar mass of Na = 23 g/mol  

Molar mass of NaCl = 58.44 g/mol

Step 3

From the balance chemical equation, 2 mol of Na produce 2 mol of NaCl. So,  

Amount of NaCl produced from the 17.25 g Na :  

= 17.25 g Na × (1 mol Na / 23 g Na) × (2 mol Na...