Question

For the reaction shown, calculate the number of grams of product from 56.7 grams of iron and sufficient chlorine. Enter your answer with the correct significant figures. Do not include units with your answer.

2Fe (s) + 3Cl2 (g) = 2FeCl3 (s)

Answer 1

164.67 grams of product FeCl₃ are produced from 56.7 grams of iron and sufficient chlorine.

Step-by-step explanation:

The balanced reaction is:

2 Fe (s) + 3 Cl₂ (g) ⇒ 2 FeCl₃ (s)

By stoichiometry of reaction (that is, the relationship between the amount of reagents and products in a chemical reaction) the following amounts of reagents and product participate in the reaction:

• Fe: 2 moles
• Cl₂: 3 moles
• FeCl₃: 2 moles

Being:

• Fe: 55.85 g/mole
• Cl: 35.45 g/mole

the molar mass of the compounds participating in the reaction is:

• Fe: 55.85 g/mole
• Cl₂: 2*35.45 g/mole= 70.9 g/mole
• FeCl₃: 55.85 g/mole + 3*35.45 g/mole= 162.2 g/mole

Then, by stoichiometry of the reaction, the following mass amounts of the compounds participate:

• Fe: 2 moles* 55.85 g/mole= 111.7 g
• Cl₂: 3 moles* 70.9 g/mole= 212.7 g
• FeCl₃: 2 moles* 162.2 g/mole= 324.4 g

Then you can apply the following rule of three: if 111.7 grams of Fe produce 324.4 grams of FeCl₃, 56.7 grams of Fe, how much mass of FeCl₃ will it form?

`mass of FeCl_(3) =(56.7 grams of Fe*324.4 grams of FeCl_(3) )/(111.7 grams of Fe)`

mass of FeCl₃= 164.67 grams

164.67 grams of product FeCl₃ are produced from 56.7 grams of iron and sufficient chlorine.