Carbon disulfide and carbon monoxide are produced when...

Carbon disulfide and carbon monoxide are produced when carbon is heated with sulfur dioxide. $$ 5 \mathrm{C}(s)+2 \mathrm{SO}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CS}_{2}(l)+4 \mathrm{CO}(g) $$ a. How many moles of $\mathrm{C}$ are needed to react with $0.500 \mathrm{~mol}$ of $\mathrm{SO}_{2}$ ? b. How many moles of $\mathrm{CO}$ are produced when $1.2 \mathrm{~mol}$ of $\mathrm{C}$ reacts? c. How many moles of $\mathrm{SO}_{2}$ are required to produce $0.50 \mathrm{~mol}$ of $\mathrm{CS}_{2}$ ? d. How many moles of $\mathrm{CS}_{2}$ are produced when $2.5 \mathrm{~mol}$ of $\mathrm{C}$ reacts?

Carbon disulfide and carbon monoxide are produced when carbon is heated with sulfur dioxide.
$$
5 \mathrm{C}(s)+2 \mathrm{SO}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CS}_{2}(l)+4 \mathrm{CO}(g)
$$
a. How many moles of $\mathrm{C}$ are needed to react with $0.500 \mathrm{~mol}$ of $\mathrm{SO}_{2}$ ?
b. How many moles of $\mathrm{CO}$ are produced when $1.2 \mathrm{~mol}$ of $\mathrm{C}$ reacts?
c. How many moles of $\mathrm{SO}_{2}$ are required to produce $0.50 \mathrm{~mol}$ of $\mathrm{CS}_{2}$ ?
d. How many moles of $\mathrm{CS}_{2}$ are produced when $2.5 \mathrm{~mol}$ of $\mathrm{C}$ reacts?

Key Concepts

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It involves using the balanced chemical equation to determine how many moles, grams, or particles of one substance are needed or produced from a given amount of another substance.

Balanced Chemical Equations

A balanced chemical equation accurately represents the conservation of mass by having an equal number of atoms for each element on both the reactant and product sides. The coefficients in the equation indicate the mole ratios that are essential for calculating the amounts of substances involved in the reaction.

Molar Ratios

Molar ratios are derived from the coefficients in a balanced chemical equation and express the proportionate amounts of reactants and products. These ratios are used to convert between moles of different substances in a reaction, enabling the calculation of unknown quantities based on a given amount of a substance.

Dimensional Analysis

Dimensional analysis is a mathematical technique used to convert units and solve problems involving measurements. In stoichiometry, it allows for the systematic conversion of moles of one substance to moles of another using conversion factors derived from molar ratios, ensuring that calculations are consistent with the units involved.

Transcript

00:01 Okay, so this question is asking us about the reaction of carbon and sulfur dioxide to form carbon di sulfide and carbon monoxide.

00:09 And so the reaction is five carbon in solid form is reacting with sulfur dioxide in gas form to produce with some heat.

00:30 Um yeah, produce carbon di sulfide and a liquid form.

00:42 Oh, that is not what i meant to do.

00:45 Mhm.

00:46 Carbon di sulfide in a liquid form and carbon monoxide in a gas form.

00:58 All right.

00:59 And so it's asking us in part a how many moles of carbon are going to be needed to react with .5 moles of of sulfur dioxide.

01:13 And so, basically what we're going to do here is we were we were given and we started off with 0.5 malls um sulfur dioxide and it's asking us how many moles of carbon are needed to react with all of this .5 moles.

01:38 Um and so what we're gonna do is we have to find the multiple factor between um carbon and sulfur dioxide.

01:45 And so to do that, we're just gonna look at the coefficients given in this balanced chemical reaction.

01:50 And we're just going to relate them to each other, find the ratio between them.

01:53 And since moles of sulfur dioxide was given to us, we want to cancel this out.

01:58 So, because we want the moles of carbon.

01:59 So our moles of sulfur dioxide is going to go on the bottom and our mole's of carbon is going to go on the top.

02:13 And so we see that two moles of sulfur dioxide.

02:17 We just grabbed this coefficient and put it right down here, goes with five moles of carbon and once again we just grabbed that right from there.

02:30 And so now what we see is that our moles of sulfur dioxide cancel out.

02:36 And our unit that we are left with his moles of carbon.

02:41 And so what we're gonna do is we're gonna take 0.5 and we're going to multiply it by five and then divide by two.

02:47 We're just going to take this fraction this ratio and multiply it by the starting amount that we were given.

02:52 And so 0.5 times 5/2 is going to give us 1.25 moles of carbon needed to react with .5 moles of sulfur dioxide.

03:09 Alright in question be they're asking us how many moles of carbon monoxide are produced from 1.2 moles of carbon reacts.

03:18 So the starting amount that we are given is 1.2 moles of carbon.

03:25 They're asking us for the relationship between moles of carbon and moles of carbon monoxide.

03:32 And so once again, we want to get rid of these moles of carbon and we want uh moles of carbon monoxide, which means our moles of carbon monoxide are going to be on top and our moles of carbon is going to be on the bottom so that these units will cancel out.

03:47 And we are given moles of carbon monoxide.

03:50 And so we can see we're just going to grab once again from the top that are moles of carbon is five.

03:58 I'm just gonna grab that coefficient and our moles of carbon monoxide is four...

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