Analyze Tetraphosphorus trisulphide (P4 S3) is used in the match heads of some matches. It is pr

Analyze Tetraphosphorus trisulphide (P4 S3) is used in the...

Analyze Tetraphosphorus trisulphide $\left(P_{4} S_{3}\right)$ is used in the match heads of some matches. It is produced in the reaction $8 \mathrm{P}_{4}+3 \mathrm{S}_{8} \rightarrow 8 \mathrm{P}_{4} \mathrm{S}_{3}$ . Determine which of the following statements are incorrect, and rewrite the incorrect statements to make them correct. \begin{equation} \begin{array}{l}{\text { a. } 4 \text { mol } P_{4} \text { reacts with } 1.5 \text { mol } S_{8} \text { to form } 4 \text { mol } P_{4} S_{3} \text { . }} \\ {\text { b. Sulfur is the limiting reactant when } 4 \text { mol } P_{4} \text { and } 4 \text { mol } S_{8} \text { react. }} \\ {\text { c. } 6 \text { mol } P_{4} \text { reacts with } 6 \text { mol } S_{8} \text { forming } 1320 \text { g } P_{4} S_{3} \text { . }}\end{array} \end{equation}

Analyze Tetraphosphorus trisulphide $\left(P_{4} S_{3}\right)$ is used in the match heads of some
matches. It is produced in the reaction $8 \mathrm{P}_{4}+3 \mathrm{S}_{8} \rightarrow 8 \mathrm{P}_{4} \mathrm{S}_{3}$ . Determine which of the following statements are incorrect, and rewrite the incorrect statements to make them correct.
\begin{equation}
\begin{array}{l}{\text { a. } 4 \text { mol } P_{4} \text { reacts with } 1.5 \text { mol } S_{8} \text { to form } 4 \text { mol } P_{4} S_{3} \text { . }} \\ {\text { b. Sulfur is the limiting reactant when } 4 \text { mol } P_{4} \text { and } 4 \text { mol } S_{8} \text { react. }} \\ {\text { c. } 6 \text { mol } P_{4} \text { reacts with } 6 \text { mol } S_{8} \text { forming } 1320 \text { g } P_{4} S_{3} \text { . }}\end{array}
\end{equation}

Key Concepts

Balanced Chemical Equation

A balanced chemical equation represents the conservation of mass and atoms during a chemical reaction by having an equal number of atoms of each element on both sides of the equation. This concept ensures that the stoichiometry of the reaction is correctly represented, which is essential for accurately determining the mole ratios between reactants and products.

Mole Ratio

The mole ratio is derived from the coefficients in a balanced chemical equation and indicates the proportion in which reactants combine and products form. It is fundamental for converting between the amounts of substances involved in a reaction, enabling the prediction of how much product will be produced from given amounts of reactants.

Limiting Reactant

The limiting reactant is the substance that is completely consumed in a chemical reaction, thereby limiting the amount of product that can be formed. Determining the limiting reactant involves comparing the mole ratios of the reactants to the ratios required by the balanced equation, which is critical for stoichiometric calculations.

Stoichiometric Calculations

Stoichiometric calculations involve using the mole ratios from a balanced chemical equation to calculate the quantities of reactants required or products formed. This includes converting between moles, mass, and sometimes volume, which is necessary for accurately interpreting chemical reactions in practical scenarios.

Mass-Mole Conversion

Mass-mole conversion is the process of converting the mass of a substance to moles (or vice versa) using the substance's molar mass. This conversion is crucial in stoichiometry for linking laboratory measurements (mass) to the theoretical mole ratios used in chemical equations.

Transcript

00:01 In this question, we are given the balanced equation for the reaction between phosphorus and sulfur, which produces tetraphosphorus trisulfide, which is a component of match heads.

00:43 Given this balanced equation of this reaction, we have to to determine whether three statements that are given are correct or incorrect.

00:58 And if they are incorrect, we have to make them correct.

01:03 We have to rewrite them the correct way.

01:08 So the first statement is saying that four moles of phosphorus react with 1.

01:22 For moles of sulfur to produce four moles of tetraposphorus triad.

01:37 Okay? now, the best way to approach this question is to look at the ratios.

01:49 Okay? so if we compare phosphorus to sulfur to sulfur, the ratio, the ratio is 8 moles of phosphor to 3 moles of sulfur.

02:09 If this is the ratio, the stoichiometric ratio, mole ratio, then this is correct, because 8 to 3 is equivalent to 4 to 1 .5.

02:27 Just if you do the math, right? you realize that if you divide, so you have here, 8.

02:34 Moles of phosphorus to three moles of sulfur.

02:43 If you divide the numerator and the denominator by two, you're gonna get four more of phosphorus to 1 .5 moles of sulfur.

03:00 So this is correct.

03:03 Now to determine if this is or this is or the the four modes that we are told are obtained, are formed of tetrafosphorus, tetrafosulosephyl sulfide, we look at the ratio, right? so eight, the ratio based on phosphorus, because we know this is correct, this ratio is correct, we can use either phosphorus or sulfur to compare with the product.

03:34 So let's say that we wanna use the phosphorus, eight modes of phosphorus, react to produce 8 moles of tetraposphorus triad sulfide.

03:46 And if we are told that 4 moles produce 4 most of phosphorus, produce 4 most of the product, then this statement is correct.

03:56 So in summary, a is correct, and we don't need to make any correction.

04:04 The next statement says that sulfur is the limited reactant when four moles, so i'm going to write the equation again here, when four moles of phosphorus react with four moles of sulfur.

04:41 We already know, they're saying that sulfur is the limiting reactant.

04:50 We already established the relationship between the mole ratio between phosphorus and sulfur.

04:57 And we say that eight moles of phosphorus must react with three moles of sulfur.

05:14 Now we need to compare this ratio, which is the theoretical ratio, to the experimental ratio, to determine which one is exactly the limiting reagent.

05:26 The value of this ratio is 8 divided by 3.

05:33 Which is 2 .6...

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