Question

For the reaction: 4Fe$_{(s)}$ + 3O$_{2(g)}$ ightarrow 2Fe$_2$O$_{3(s)}$ a. What mass (g) of oxygen gas would be required to fully react with 784 mg of iron? b. What mass (g) of ferric oxide would be produced in this reaction with 784 mg of iron?

          For the reaction: 4Fe$_{(s)}$ + 3O$_{2(g)}$ 
ightarrow 2Fe$_2$O$_{3(s)}$
a. What mass (g) of oxygen gas would be required to fully react with
784 mg of iron?
b. What mass (g) of ferric oxide would be produced in this reaction
with 784 mg of iron?

For the reaction: 4Fe(s) + 3O2(g)
ightarrow 2Fe2O3(s)
a. What mass (g) of oxygen gas would be required to fully react with
784 mg of iron?
b. What mass (g) of ferric oxide would be produced in this reaction
with 784 mg of iron?

Added by Aaron V.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Joshua Klint

10/21/2023

Step 1

The molar mass of Fe is 55.85 g/mol. Since we have 784 mg, we need to convert it to grams: 784 mg * (1 g / 1000 mg) = 0.784 g Now, we can find the moles of Fe: moles of Fe = (0.784 g) / (55.85 g/mol) = 0.01404 mol From the balanced equation, we can see that 4 Show more…

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