Determine all possible mole ratios for the following...

Determine all possible mole ratios for the following balanced chemical equations. \begin{equation} \begin{array}{l}{\text { a. } 4 \mathrm{Al}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{s})} \\ {\text { b. } 3 \mathrm{Fe}(\mathrm{s})+4 \mathrm{H}_{2} \mathrm{O}\left(\mathrm{l} \rightarrow \mathrm{Fe}_{3} \mathrm{O}_{4}(\mathrm{s})+4 \mathrm{H}_{2}(\mathrm{g})\right.} \\ {\text { c. } 2 \mathrm{HgO}(\mathrm{s}) \rightarrow 2 \mathrm{Hg}(1)+\mathrm{O}_{2}(\mathrm{g})}\end{array} \end{equation}

Determine all possible mole ratios for the following balanced chemical equations.
\begin{equation}
\begin{array}{l}{\text { a. } 4 \mathrm{Al}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{s})} \\ {\text { b. } 3 \mathrm{Fe}(\mathrm{s})+4 \mathrm{H}_{2} \mathrm{O}\left(\mathrm{l} \rightarrow \mathrm{Fe}_{3} \mathrm{O}_{4}(\mathrm{s})+4 \mathrm{H}_{2}(\mathrm{g})\right.} \\ {\text { c. } 2 \mathrm{HgO}(\mathrm{s}) \rightarrow 2 \mathrm{Hg}(1)+\mathrm{O}_{2}(\mathrm{g})}\end{array}
\end{equation}

Key Concepts

Stoichiometry

Stoichiometry is the area of chemistry that deals with calculating the quantitative relationships between reactants and products in chemical reactions. It relies on the balanced chemical equation to determine the exact amounts of each substance involved, which is essential for predicting yield, scaling reactions, and conducting laboratory experiments.

Mole Ratios

Mole ratios are the proportional relationships between the moles of reactants and products that are deduced directly from the coefficients in a balanced chemical equation. These ratios allow chemists to convert from the mass of a substance to moles and subsequently predict how much of each reactant is needed or product is formed, thereby playing a key role in stoichiometric calculations.

Balanced Chemical Equations

These are chemical equations in which the number of atoms for each element is the same on both the reactant and product sides of the equation, reflecting the law of conservation of mass. This concept is fundamental in ensuring that all chemical reactions adhere to the principle that matter is neither created nor destroyed during a reaction.

Transcript

00:01 In this question, we need to provide the all possible mole ratios given three balanced chemical reactions or chemical equations.

00:17 So in the first one, all possible molar ratios are four moles of aluminum will produce two moles of aluminum oxide.

00:33 3 moles of oxygen will produce 2 moles of aluminum oxide and 4 moles of aluminum will react with 3 moles of oxygen and we can also reverse this ratio we can say 2 moles of aluminum are produced when four moles of aluminum react.

01:22 Two moles of aluminum oxide are produced when three moles of oxygen react.

01:33 And three moles of oxygen react with four moles of aluminum.

01:45 Okay? in the second equation, we have the possible mole ratios are three moles of iron will produce one mole of iron two oxide iron two iron two item three because the chart here is negative eight so we have positive eight eight divided by three it's a number between two and three okay so it's iron 2, 3 oxide.

02:49 The other possible ratio is 3 mol of iron, will produce 4 moles of hydrogen.

03:05 Another one would be 4 moles of water, will produce 1 mole of iron oxide, item 2, 3 oxide.

03:28 4 moles of water will produce 4 moles of hydrogen.

03:39 Another possible ratio is three moles of iron react with four molds of water.

04:00 And the last possible ratio would be one mole of iron to three oxide is produced in conjunction with four moles of hydrogen.

04:25 Okay? and again, we can reverse all of this ratio...

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