A chemist reacted 11.50 grams of sodium metal with an excess amount of chlorine gas. The chemical reaction that occurred is shown. 2Na + Cl2 → 2NaCl

If the actual yield of the reaction is 24.85 g of NaCl, what is the percent yield? Show your work including, the use of stoichiometric calculations and conversion factors.

24.85 g

Explanation:

From the equation;  1 mole of Sodium metal produces 2 moles sodium chlorides This means;  23 g of Na will produce 116.88 g of NaCl  Therefore;  11.5 g will generate;   = (11.5 × 116.88)/23 =  58.44 g of NaCl  But;  Percentage yield = (Actual yield/Theoretical yield)× 100%  85 /100 = Actual yield /58.44 g Thus; Actual yield = 0.85 × 58 = 24.85 g

answer: i have one answer

acids are substances that ionize (break off) in an aqueous solution to produce hydrogen (h+) ions

explanation:

hope this and sorry i could only come up with one answer!