The reaction between solid sodium and iron(llI) oxide is one...

The reaction between solid sodium and iron(llI) oxide is one in a series of reactions that inflates an automobile airbag: $6 \mathrm{Na}(\mathrm{s})+\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{s}) \rightarrow 3 \mathrm{Na}_{2} \mathrm{O}(\mathrm{s})+2 \mathrm{Fe}(\mathrm{s}) .$ If 100.0 $\mathrm{g}$ of $\mathrm{Na}$ and 100.0 $\mathrm{g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3}$ are used in this reaction, determine the following. \begin{equation} \begin{array}{l}{\text { a. limiting reactant }} \\ {\text { b. reactant in excess }} \\ {\text { c. mass of solid iron produced }} \\ {\text { d. mass of excess reactant that remains after the reaction is complete }}\end{array} \end{equation}

The reaction between solid sodium and iron(llI) oxide is one in a series of reactions that
inflates an automobile airbag: $6 \mathrm{Na}(\mathrm{s})+\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{s}) \rightarrow 3 \mathrm{Na}_{2} \mathrm{O}(\mathrm{s})+2 \mathrm{Fe}(\mathrm{s}) .$ If 100.0 $\mathrm{g}$ of $\mathrm{Na}$
and 100.0 $\mathrm{g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3}$ are used in this reaction, determine the following.
\begin{equation}
\begin{array}{l}{\text { a. limiting reactant }} \\ {\text { b. reactant in excess }} \\ {\text { c. mass of solid iron produced }} \\ {\text { d. mass of excess reactant that remains after the reaction is complete }}\end{array}
\end{equation}

Key Concepts

Mass-Mole Conversions

Mass-mole conversions involve using the molar mass of a substance to convert between mass (grams) and the amount of substance in moles. This conversion is fundamental in stoichiometric calculations, enabling the quantitative analysis of reactants and products.

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction in which the number of atoms of each element is equal on both the reactant and product sides. It is crucial for understanding the stoichiometric relationships between reactants and products, ensuring that mass is conserved during the reaction.

Stoichiometry

Stoichiometry involves the calculation of relative quantities of reactants and products in a chemical reaction. It uses the balanced chemical equation to determine how many moles of each substance participate in the reaction, which is essential for predicting the outcomes of chemical processes.

Limiting Reactant

The limiting reactant is the chemical reagent that is completely consumed in a reaction, thereby determining the maximum amount of product that can be formed. Identifying the limiting reactant allows one to predict the theoretical yield of the reaction.

Excess Reactant

An excess reactant is any reactant that remains after the limiting reactant has been completely consumed. Calculating the amount of excess reactant left over after a reaction is important for process efficiency and cost analysis.

Transcript

00:01 In this problem, we are given the balanced equation for the reaction between sodium and iron -3 oxide.

00:14 I'm going to write it down right here.

00:19 The reaction between these two reactants produces sodium oxide and iron.

00:35 Okay? the first question that we need to answer is to determine which one is a limiting reagent if you mix 100 grams of sodium with 100 grams of iron 3 oxide.

00:52 To determine which one is a limiting reagent between these two reactants, we need to first establish the mold relationship and then convert that more relationship to a mass relationship.

01:08 Relationship or ratio to see which one is not enough in the reaction or and which one is in excess.

01:18 So the mole ratio is 6 moles of sodium react with one mole of ion 3 oxide based on this balanced equation.

01:31 So let's establish the ratio and then see which one is the limiting reagent.

01:40 So again, six moles of sodium reacts with one mole of iron three oxide.

01:51 And now we convert this to grams to grams, a mass ratio.

02:01 The atomic weight of sodium is 22 .99 grams per mole.

02:10 And the molar mass of iron three oxide is two times the atomic weight of iron, which is 55 .85 plus three times the atomic weight of oxygen, which is 16.

02:33 And this is grams per mole okay and then we made these liter calculations in the numerator we have a hundred and thirty seven point nine grams moles cancelled and here we have 159 .7 grads because moles cancelled therefore we need if we have only, if we have 100 and 100, right, the relationship, sodium, the real relationship we have, the experimental relationship we have, is 100 grams of sodium to 100 grams of item 3 oxide.

04:06 Right? so, just by looking and comparing these two ratio, you realize that we don't have.

04:15 This ratio is one, right? and this ratio is less than one.

04:21 And this is the stereometric ratio.

04:23 This is the one that we have to fulfill.

04:28 Therefore, in order to make this ratio less than one, this amount has to be greater than this amount.

04:41 Therefore, iron three oxide is the limiting, okay, and therefore sodium is the reactant in excess.

05:22 Now we need to calculate the mass of iron that is produced.

05:29 Okay? so the reactant that will completely react and will determine the amount of products that will be formed is the limiting reagent, is the limiting reactant.

05:47 In this case, iron three oxide, because you have an excess of sodium.

05:55 Therefore, in order to determine the amount that is formed of iron, we are going to use iron three oxide, the reagent that is in limiting amount.

06:11 And therefore, we're going to use the mole ratio and then convert that more ratio to mass ratio between item 3 oxide and item.

06:24 Okay? so the ratio, and this would be the unknown.

06:29 The ratio is one mole of item 2 oxide...

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