Iron oxide ores, commonly a mixture of FeO and Fe2 O3, are given the general formula Fe3 O4. The

Iron oxide ores, commonly a mixture of FeO and Fe2 O3, are...

Iron oxide ores, commonly a mixture of $\mathrm{FeO}$ and $\mathrm{Fe}_{2} \mathrm{O}_{3}$, are given the general formula $\mathrm{Fe}_{3} \mathrm{O}_{4}$. They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemental hydrogen. Balance the following equations for these processes. $$\begin{aligned}\mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{H}_{2}(g) & \rightarrow \mathrm{Fe}(s)+\mathrm{H}_{2} \mathrm{O}(g) \\ \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}(g) & \rightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g)\end{aligned}$$

Iron oxide ores, commonly a mixture of $\mathrm{FeO}$ and $\mathrm{Fe}_{2} \mathrm{O}_{3}$, are given the general formula $\mathrm{Fe}_{3} \mathrm{O}_{4}$. They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemental hydrogen. Balance the following equations for these processes.
$$\begin{aligned}\mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{H}_{2}(g) & \rightarrow \mathrm{Fe}(s)+\mathrm{H}_{2} \mathrm{O}(g) \\
\mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}(g) & \rightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g)\end{aligned}$$

Key Concepts

Redox Reactions

Redox (reduction-oxidation) reactions involve the transfer of electrons between chemical species, where one substance is oxidized (loses electrons) and another is reduced (gains electrons). This concept is critical in processes such as the extraction of metals from their ores, where reducing agents are employed to convert metal oxides to elemental metals.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on the reactants side as on the products side. This concept is essential in chemistry as it reflects the law of conservation of mass, meaning that atoms are neither created nor destroyed during a chemical reaction.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It involves the use of balanced chemical equations to calculate the amount of each substance needed or produced, allowing for accurate prediction of yields and optimization of chemical processes.

Transcript

00:01 We are looking at two similar reactions of how to get elemental iron from iron ore.

00:11 And in their current state, these reactions are unbalanced, and we want to balance them.

00:19 So our first step to doing that is to count up how many of each atom, how many atoms of each element we have on either side of the reaction.

00:31 Arrow.

00:33 So i'm going to count them up.

00:35 Here i have three iron atoms, four oxygen, and two hydrogen.

00:43 Meanwhile on this side, i have one iron atom, two hydrogen atoms, and one oxygen atom.

00:55 So looking at our most complicated molecule first are fe 304.

01:04 I notice i have four oxygens that on the other side i only have one.

01:12 So the first thing i'm going to try is just putting a four here, seeing what happens then.

01:22 So if i do that, then i have now four oxygens on the other side, which is good.

01:29 But now i have eight hydrogens on this side and only two on my reactant side.

01:36 So pretty simple way to match those up is to also put a four here.

01:45 So now we have eight oxygens on either side.

01:49 Excuse me, four oxygens, eight hydrogens on either side.

01:55 And i have three irons here and only one here, but i can simply put a three here, two, now have three irons here.

02:07 So just to confirm, three irons, three irons, four oxygens, four oxygens, eight hydrogens, eight hydrogens.

02:17 So this is my final answer.

02:22 I'm going to turn these green.

02:24 So i remember that i am good to go.

02:31 And this is a balanced equation.

02:40 Now my next step is to balance the next equation.

02:45 Here i have three irons.

02:50 I have four plus one.

02:52 One over here of oxygen.

02:55 So i have a total of five oxygen molecule, not molecule, sorry, atoms.

03:02 And i have one carbon atom...

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