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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?

$$76.6 \%$$

Chemistry 101

Chapter 3

Mass Relationships in Chemical Reactions

Chemical reactions and Stoichiometry

University of Central Florida

University of Maryland - University College

Lectures

04:02

A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Chemical reactions can be either spontaneous, requiring no input of energy, or non-spontaneous, typically following the input of some type of energy, such as heat, light or electricity. Chemical reactions are usually characterized by a chemical change, and they yield one or more products after the reaction is complete. Chemical reactions are described with chemical equations, which symbolically present the starting materials, end products, and sometimes intermediate products and reaction conditions. Chemical reactions happen at a characteristic reaction rate at a given temperature and chemical concentration. Typically, reaction rates increase with increasing temperature because there is more thermal energy available to reach the activation energy necessary for breaking bonds between atoms.

08:02

In chemistry, a combination reaction is a chemical reaction in which two or more reactants combine to form more than one product. In a decomposition reaction, one reactant splits into two or more products.

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sort of this problem. We have the formation reaction of they sold, fight they chloride and you want to find the theoretical yield as well as he actually all of the reaction. So we know that the balanced reaction that we're dealing with is the following. The first thing that we want to get before you get into the initial quantities is he one actually find the more masses of all of the rail relevant substances. So first we have That's a well, this is just eight suffers and each sulfur Adam has an atomic weight of 32 point of seven. So when you multiply this through, we'll get 2 56 0.56 grams promote. Then we have sealed too well. The atomic massive chlorine Adam is 35.45 when you have two of them, so any multiplied together, we'll get 70 I know grams per mole. And finally, for Salford I chloride. We have to sulphur atoms and you have to Corinne Adams. So that's just two times 32 point of seven and two times 35.45 And then multiply those two together you will get 1 35 no. Four grams promote. 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 So we can then choose which substance to bathe Oliver Streak younger tree on. Let's first start with s eight and find how many moles of seal to required to react with all of it. So we know that we are given for initial quantity our initial quantities. You are given four point no six grams of estate as well as 6.24 grams of seal too. So you have four point no. Six grams of s it. Well, first, we just divide by the molar mass so we can get moles of s eight when he calculated that to be to 56.56 grams per one more the feet and now they want to find the multiple ratio. Well, we see that in order to react with one mole of s eight, four molds of chorine gas required to the mole to mole ratio is 4 to 1. And when you multiply this through, we'll see that 0.0 633 Moles of seal to are required to react with all of our sulfur. So now we want to find how much or how much chorine gas do we have to begin with? Well, we know that we have 6.24 grams. Of course, gas. No need to do is just divide by the more mass which we calculated to be 70.9 grams for one more will feel too. And we will see that we have 0.80 moles of steel to so now that we see that the amount of seal to that we have is greater than the amount of co two that we need to react with all this offer, Sulfur is a limiting reactant. And that's ah reacting that we're gonna base all of her story geometry off now. So now we know that's all fairies alone. You reckon you want to find the theoretical yield for they sulphur chloride? So we have 4.6 grams of sulfur. We then divide by the molar mass to get moles of sulfur who take the multiple ratio of sulphur di chloride of die sulphur to chlorine and sulfur. You look at the equation we see that four moles of sisal for declarative form with one mole of sulfur, so the multiple ratio is 4 to 1. And then finally we multiply by the more mass, which we calculated at the very beginning to be 1 34.4 Now, when you multiply all these quantities together, we'll get that the theoretical yield of they suffered a chloride was 8.55 grams. Does that answer is the first part of this question. Now we want to find the actual percent yield. So the question tells us that 6.55 grams of they sulfur deployed was the actual yield, and we know that the formula 4% yield is actual or extra mental over theoretical multiplied by 100. So we have 6.55 That's experimental value. If 8.55 as our theoretical value, multiply these two quantities and we get that air yield is 76 0.6% and that is the final answer

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