Question

1. Rust, Fe2O3, form from the reaction of iron and oxygen in the following equation:

Fe(s)+O2(g)→Fe2O3(s)

a. Write the balanced equation of the reaction.

b. What is the mole-mole ratio of Fe to Fe2O3?

c. How many moles of Fe2O3 is produced from 39.4 moles of Fe?

d. What is the molar mass of Fe2O3?

e. How many grams of O2 are needed to produce 29.8 g of Fe2O3?


2. Given the decomposition reaction: 2 KClO3(s)→2KCl(s)+3 O2(g)

a. What is the mole-mole ratio of KClO3 to O2?

b. What is the molar mass of KClO3?

c. How many moles of KClO3 are needed to produce 36.6 moles of O2?

d. How many grams of KCl are produced from an initial mass of 568.4 g KClO3?

Answer 1

Answer:

Balanced equation: 4 Fe(s) + 3 O2(g) = 2 Fe2O3(s)

Reaction stoichiometry Limiting reagent

Compound # Molar Mass

Fe(s) 4 55.845

O2(g) 3 31.9988

Fe2O3(s) 2 159.6882