The balanced equation for a reaction in the process of...

The balanced equation for a reaction in the process of reducing iron ore to the metal is $$ \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{s})+3 \mathrm{CO}(\mathrm{g}) \longrightarrow 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_{2}(\mathrm{g}) $$ (a) What is the maximum mass of iron, in grams, that can be obtained from $454 \mathrm{g}(1.00 \mathrm{lb})$ of iron(III) oxide? (b) What mass of $\mathrm{CO}$ is required to react with $454 \mathrm{g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3} ?$

The balanced equation for a reaction in the process of reducing iron ore to the metal is
$$
\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{s})+3 \mathrm{CO}(\mathrm{g}) \longrightarrow 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_{2}(\mathrm{g})
$$
(a) What is the maximum mass of iron, in grams, that can be obtained from $454 \mathrm{g}(1.00 \mathrm{lb})$ of iron(III) oxide?
(b) What mass of $\mathrm{CO}$ is required to react with $454 \mathrm{g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3} ?$

Key Concepts

Balanced Chemical Equation

A balanced chemical equation indicates the precise correspondence between the number of atoms of each element on the reactant side to those on the product side. This fundamental concept ensures the law of conservation of mass is maintained and provides the stoichiometric ratios needed to calculate the amounts of reactants and products in a chemical reaction.

Mole Concept

The mole is a unit used to express amounts of a chemical substance, representing a specific number (Avogadro's number) of particles. This concept allows chemists to relate masses of substances to the number of molecules or atoms involved, which is crucial in stoichiometric calculations.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. It serves as the conversion factor between the mass of a substance and the number of moles, which is essential in quantifying reactants and products in chemical reactions.

Stoichiometry

Stoichiometry involves the quantitative relationships derived from a balanced chemical equation, enabling calculations of the required amounts of reactants or the expected amounts of products. It uses the mole ratios from the balanced equation to convert between moles and mass of substances.

Transcript

00:01 Hello friends, in this video we will learn how to do some stoichiometric calculations.

00:07 So as you can see, you have been given a chemical equation in front of you in which iron 3 oxide is reacting with carbon monoxide to give iron and carbon dioxide.

00:20 Okay, so in this, we have to solve two questions in this.

00:26 So the first question is we have to find out the maximum mass of iron.

00:32 Maximum mass of iron produced using 454 grams of iron 3 oxide okay and the next question we need to answer is the mass of carbon monoxide produced mass of carbon monoxide produced not produced required so mass of carbon monoxide required mass of carbon monoxide required mass of carbon monoxide required to react with 454 grams of iron 3 oxide.

01:32 So it's simple.

01:33 So there are two questions.

01:35 We have been given an equation.

01:37 We need to find out what is the maximum mass of iron which is produced when we use 454 grams of iron 3 oxide.

01:45 And also we have to find out what is the mass of carbon monoxide required to react with 454 grams of fe203.

01:56 Okay, so before we go ahead, we can just check whether our equation is balanced or not.

02:04 So we can see here, there are two atoms of iron on the reactant side and two atoms of iron on the product size as well.

02:13 Then there are six atoms of oxygen on the reactant side and six atoms of oxygen on the product side.

02:19 Then three atoms of carbon on the reactin side and three atoms of carbon on the product side.

02:24 So this equation is perfectly balanced.

02:27 Now the next step we have to do is we have to find the molar masses of all the compounds here.

02:33 So how do we find the molar masses? so we can refer to the periodic table.

02:38 See the mass of each of like we can check the mass of one atom of each element.

02:46 And then we have to add it up.

02:48 So for example, so iron oxide is 2 into the atomic mass of atom.

02:55 Iron is 56 so it will be 2 into 56 plus 3 into 16 because the atomic mass of oxygen is 16 right so this will give us the molar mass of iron 3 oxide so if we do this it comes out to 160 grams per mole so similarly we can add up for carbon monoxide as well so carbon monoxide comes to 20 grams per mole and iron is 56 grams and carbon monoxide carbon dioxide is 44 grams okay so you can see the coefficients here so it means during the reaction three multiplied or three moles of carbon monoxide is used up so basically three into 28 grams of carbon monoxide is used up similarly two multiplied by 56 grams of iron is produced also 3 multiplied by 44 grams of carbon dioxide is produced right so let's get the final calculation here so 160 gram of fe 203 is reacting with 3 into 28 so let's calculate what is 3 into 28 so 3 multiplied by 28 which is 84 so it reacts with 84 grams of carbon monoxide.

04:43 Okay, and then it reacts with 50, it produces 56 into 2...

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