Disulfide dichloride (S2 Cl2) is used in the vulcanization of rubber, a process that prevents th

Disulfide dichloride (S2 Cl2) is used in the vulcanization...

Disulfide dichloride $\left(\mathrm{S}_{2} \mathrm{Cl}_{2}\right)$ is used in the vulcanization of rubber, a process that prevents the slippage of rubber molecules past one another when stretched. It is prepared by heating sulfur in an atmosphere of chlorine:$$\mathrm{S}_{8}(l)+4 \mathrm{Cl}_{2}(g) \longrightarrow 4 \mathrm{~S}_{2} \mathrm{Cl}_{2}(l)$$What is the theoretical yield of $\mathrm{S}_{2} \mathrm{Cl}_{2}$ in grams when $4.06 \mathrm{~g}$ of $\mathrm{S}_{8}$ are heated with $6.24 \mathrm{~g}$ of $\mathrm{Cl}_{2} ?$ If the actual yield of $\mathrm{S}_{2} \mathrm{Cl}_{2}$ is $6.55 \mathrm{~g}$, what is the percent yield?

Key Concepts

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by dividing the actual yield (the amount of product actually obtained) by the theoretical yield and then multiplying by 100. This percentage indicates how close the reaction came to its maximum possible output.

Theoretical Yield

The theoretical yield is the maximum amount of product that could be produced in a reaction, as predicted by stoichiometry, assuming that the reaction proceeds perfectly with complete conversion of the limiting reagent. It serves as a benchmark for understanding the efficiency of the reaction.

Limiting Reagent

The limiting reagent is the reactant that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reagent is crucial for accurately calculating the theoretical yield of the reaction.

Balanced Chemical Equation

A balanced chemical equation provides the stoichiometric relationship between reactants and products in a chemical reaction. By ensuring that the number of atoms of each element is conserved, it enables chemists to determine the proportions in which substances react and the corresponding amounts of products formed.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction as dictated by the balanced chemical equation. It allows the calculation of how much product can be formed from given amounts of reactants, based on their mole ratios.

Mole Concept

The mole concept is a fundamental idea in chemistry that links the mass of a substance to the number of its constituent particles using the substance's molar mass. This concept allows the conversion between grams and moles, which is essential for quantifying substances in a chemical reaction and making stoichiometric calculations.

Transcript

00:01 So for this problem, we have the formation reaction of disulfide dichloride, and we want to find the theoretical yield as well as the actual yield of the reaction.

00:11 So we know that the balanced reaction that we are dealing with is the following.

00:21 So the first thing that we want to do before you get into the initial quantities is you want to actually find the molar masses of all the relevant substances.

00:30 So first, we have s8.

00:33 Well, this is just 8 sulfurs, and each sulfur atom has an atomic weight of 32 .07.

00:44 So when you multiply this through, we'll get 256 .0 .56 grams per mole.

00:54 Then we have cl2.

00:57 Well, the atomic mass of a chlorine atom is 35 .45, and we have two of them.

01:05 So when you multiply together, we'll get 70 grams per mole.

01:13 And finally, for sulfur di -chloride.

01:18 We have two sulfur atoms and we have two chlorine atoms.

01:25 So that's just two times 32 .07 and two times 35 .45.

01:37 And then when we multiply those two together, you will get 1 .307.

01:41 35 .04 grams per mole.

01:46 So now that we have all of the relevant molar masses for all of our substances, we can then go on to find the limiting reactant.

01:55 So we can then choose which substance to base all of our strychometry on.

01:59 So let's first start with s8 and find how many moles of cl2 are required to react with all of it.

02:07 So we know that we are given for our initial quantity, to our initial quantities.

02:12 We are given 4 .06 grams of s8 as well as 6 .24 grams of cl2.

02:29 So we have 4 .06 grams of s8.

02:36 Well first we just divide by the molar mass so we can get moles of s8.

02:41 And we calculated that to be 256 .56 grams per one mole.

02:49 Of s8.

02:52 And now we want to find the multi -mole ratio...

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