# Answer to Question #203040 in General Chemistry for Ade Irma Daniar

Question #203040

2. A student carried out a reaction between iron and hydrochloric acid to make some iron (II) chloride crystals. She started with 5.6g of iron and used an excess of hydrochloric acid.

a. Write a balanced chemical equation for the reaction!    

b. How many moles of iron did he start off with?    

c. What mass of iron (II) chloride should he have expected from this reaction?    

d. He actually obtained 9.17g of the iron (II) chloride. What was his percentage yield? 

1
Expert's answer
2021-06-07T03:15:54-0400

a)Fe + 2HCl -->> FeCl2 + H2

b) Molar Mass of iron = 55.845

= 5.6/55.845

= 0.1 m

c) Molar Mass of FeCl2 = 126.751

= 126.751 × 0.1

= 12.71g

d) 12.71-9.17

= 3.54

= 3.54/12.71 × 100

= 27.85%

Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!

#### Comments

No comments. Be the first!

### Ask Your question

LATEST TUTORIALS
New on Blog
APPROVED BY CLIENTS