Carbon disulfide, CS2 can be made from coke, C and sulfur dioxide, SO2: 3C + 2 SO2→ CS2 + CO2. If the actual yield of CS2 is 86% of the theoretical yield, what mass of coke is needed to produce 950g of CS2?

Md Ariful Islam

0 like 0 dislike
1 views
Share with your friends

1 Answers

Md Ariful Islam

Call

Since $950$ $"g"$ is the desired mass of $"CS"_2$, and the is $86%$, the theoretical yield of $"CS"_2$ is

$950$ $"g CS"_2"$ $xx 100/86 = ul(1107color(white)(l)"g CS"_2$

Now, let's convert this value to moles, using the molar mass of carbon disulfide:

$1107cancel("g CS"_2)((1color(white)(l)"mol CS"_2)/(76.14cancel("g CS"_2))) = color(red)(14.5$ $color(red)("mol CS"_2$

Now, we use the coefficients of the chemical equation to find the relative number of moles of $"C"$:

$color(red)(14.5)cancel(color(red)("mol CS"_2))((3color(white)(l)"mol C")/(1cancel("mol CS"_2))) = color(green)(43.5$ $color(green)("mol C"$

Finally, we use the molar mass of coke (carbon) to find the mass:

$color(green)(43.5)cancel(color(green)("mol C"))((12.011color(white)(l)"g C")/(1cancel("mol C"))) = color(blue)(ul(523color(white)(l)"g C"$

0 like 0 dislike
1 views
Talk Doctor Online in Bissoy App
Carbon disulphide 'CS2' . Can be made from by product SO2. The overall reaction is 5C + 2SO2 -------> CS2 + 4CO How much CS2 can be produced from 450kg of waste SO2 with excess of coke if the SO2 conversion is 82%?

$5C(s) + 2SO_2(g) rarr CS_2(g) +4CO(g)$ $"Moles of sulfur dioxide"=(450xx10^3*g)/(64.07*g*mol^-1)=7023.6*mol$ And thus, factoring in the yield AND the ......we gets..... $82%xx7023.6*molxx1/2xx76.14*g*mol^-1-=219.2*kg$ $CS_2$. The reaction turns on the stoichiometry. 1 equiv...

1 Answers 1 views
Iron can be extracted from iron(III) oxide by heating it with coke (carbon). The other product in the extraction reaction is carbon dioxide. What mass of iron is produced by reacting 550g of iron(III) oxide with 60g of coke?

Balanced Equation $"2Fe"_2"O"_3 + "3C"$$rarr$$"4Fe + 3CO"_2$ This is a limiting reactant question. The maximum amount of $"Fe"$ that can be produced is determined by the limiting reactant. We have...

1 Answers 1 views
Given the following, what is the limiting reactant? What is the theoretical yield of $Cl_2$? If the yield of the reaction is 75.5%, what is the actual yield of chlorine?

This is a limiting reactant problem. We know that we will need a balanced equation with masses, molar masses, and moles of the involved. 1. Gather all the information...

1 Answers 1 views
What is the theoretical yield and percent yield of $"AgCl"$ if $"102.6996 g CsCl"$ reacts with excess $"AgNO"_3"$? The actual yield of $"AgCl"$ is $"77.938858 g"$.

This is a double replacement (double displacement reaction). Balanced Equation $"CsCl(aq)"+"AgNO"_3("aq")$$rarr$$"CsNO"_3("aq")+"AgCl(s)"$ Molar Masses We need the molar masses of $"CsCl"$ and $"AgCl"$. $"CsCl:"$$"168.358452 g/mol"$ $"AgCl:"$$"143.3212 g/mol"$ Theoretical...

1 Answers 1 views
Methane and hydrogen sulfide form when 36g $H_2$ reacts with carbon disulfide. What is the percent yield if the actual yield of $CH_4$ is 69.8g?

In order to determine a reaction's , you need to know two things the actual yield of the reaction the theoretical yield of the reaction In...

1 Answers 1 views
If a reaction has an actual yield of 5 grams and a theoretical yield of 10 grams, what is the percent yield?

Let's define those three terms before we get started: The percent yield of a reaction is the ratio of actual yield to the theoretical yield times one-hundred percent....

1 Answers 1 views
Define the terms theoretical yield, actual yield, and percent yield. Why is the actual yield in a reaction almost always less than the theoretical yield? Can a reaction ever have 110% actual yield?

Actual yield in a reaction is almost always less than the theoretical yield, primarily because losses of the substances involved may occur anywhere in an experiment. Otherwise, there can be...

1 Answers 1 views
In an experiment to prepare a particular compound, the theoretical yield s 65.3 g and the actual yield is 56.3 g. What is the percent yield?

A reaction's is simply the number of grams of a product that you actually get for every $"100 g"$ of said product that you could theoretically get. The...

1 Answers 1 views
If the theoretical yield for a chemical reaction is 100. g and the percentage yield is 70.0%, what is the actual yield?

The actual yield is a term used to describe the amount of product that is actually produced by a given chemical reaction. By comparison, the theoretical yield is a...

1 Answers 1 views
The burning of 18.0 g of carbon produces 55.0 g of carbon dioxide. What is the theoretical yield of $CO_2$? How do you calculate the percent yield of $CO_2$?

And, given the $1:1$ $"stoichiometry,"$ $%"yield"="Moles of carbon dioxide"/"Moles of carbon"xx100%$ $=((55.0*g)/(44.01*g*mol^-1))/((18.0*g)/(12.011*g*mol^-1))xx100%=83%$

1 Answers 1 views
X