Answer to Question #141644 in Inorganic Chemistry for Rameen

Question #141644
When 10.11g of hydrochloric acid reacts with 10.3 g of aluminum hydroxide,

a. Identify the limiting reagent
b. Find the moles of the salt produced
c. Find the moles of the excess reactant used up in the reaction
d. Find the moles of the excess reactant leftover after the reaction is complete
e. Find the mass of the excess reactant leftover after the reaction is complete
f. When this reaction was completed in the lab, the percentage yield (of the salt produced) was 72.5%. What is the actual yield?
1
Expert's answer
2020-11-02T08:52:57-0500

A) The reactant that produces a lesser amount of product is the limiting reagent.  That's Hcl


B) 20.41/ 133.34

= 0.1531 moles


C) 1- 0.1531 = 0.8469moles


D) 0.8469- 0.1531 = 0.6948moles


E) 1 mole = 133.34g


0.6948moles =( (0.6948)(133.34))


= 92.64g


F) 72.5% = 92.64g


100% = ?

Therefore : = ((92.64)(100))/72.5


= 127.78g


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