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University of Toronto

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Problem 69

Bismuth oxide reacts with carbon to form bismuth metal:

$$

\mathrm{Bi}_{2} \mathrm{O}_{3}(s)+3 \mathrm{C}(s) \longrightarrow 2 \mathrm{Bi}(s)+3 \mathrm{CO}(g)

$$

When 283 g of $\mathrm{Bi}_{2} \mathrm{O}_{3}$ reacts with excess carbon, how many

(a) moles of $\mathrm{Bi}_{2} \mathrm{O}_{3}$ react and (b) moles of Bi form?

Answer

$\mathrm{n}\left(\mathrm{Bi}_{2} \mathrm{O}_{3}\right)=0,607 \mathrm{mol}$

$\mathrm{n}(\mathrm{Bi})=1,22 \mathrm{mol}$

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## Discussion

## Video Transcript

Who are we keeping the reaction between? Give this with all site and carbon. So we have 2 83 gram or business Offsay going to wear with excess carbon. So reformed Smith also carbon downside. So for product door question, we want to file the number one most of different oxide being reacted. And also people would be the number one most off if it thean polio's. Okay, so first of all, we have to find the numbers off more office with oxide. So we're going to take the, uh, masks which were keeping it to 80 If we graham the 2 83 Graham divided by them with a masterpiece Smith Ah Hokusai So the modem ASAP. Izmit also I will be, um this also So we are going to two times Ah too. And I Plus because we have to this myth and then flew the oxygen So three times 16 at the whole unit were Quimper moves so we can find the mambo moves to side too. And we will We will have syrup on 607 most Oh, piss me Fox. Okay, so the number move a piece with me inform is that we are looking at the reaction is everything in balance? So we're looking We're looking at the coefficient, and then we can know that their mother away show So the moon away show between the business also. And, uh, this myth will be 1 to 2 Big the officials one here, the coefficients one for business off site. And also to who? For Christmas. So it's 1 to 2. When we have one more off base with Fox, I report goes to more business. So therefore Ah, the ah number more visibly to time series. So points six or seven and then they will be close to one point. Ah ah! To one most for this myth.

## Recommended Questions

Pure bismuth can be produced by the reaction of bismuth

oxide with carbon at high temperatures.

$$2 \mathrm{Bi}_{2} \mathrm{O}_{3}+3 \mathrm{C} \rightarrow 4 \mathrm{Bi}+3 \mathrm{CO}_{2}$$

How many moles of $\mathrm{Bi}_{2} \mathrm{O}_{3}$ reacted to produce 12.6 $\mathrm{mol}$

of $\mathrm{CO}_{2} ?($Chapter 11$)$

Iron(III) oxide reacts with carbon monoxide according to the equation:

$$\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)$$

A reaction mixture initially contains 22.55 $\mathrm{g} \mathrm{Fe}_{2} \mathrm{O}_{3}$ and 14.78 $\mathrm{gCO}$ .

Once the reaction has occurred as completely as possible, what mass

(in $\mathrm{g} )$ of the excess reactant remains?

Iron(III) oxide reacts with carbon monoxide according to the equation:

$$\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)$$

A reaction mixture initially contains 22.55 $\mathrm{g} \mathrm{Fe}_{2} \mathrm{O}_{3}$ and 14.78 $\mathrm{g}$ CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Chromium metal reacts with oxygen to give chromium(III) oxide, $\mathrm{Cr}_{2} \mathrm{O}_{3}$

(a) Write a balanced equation for the reaction.

(b) If a piece of chromium has a mass of $0.175 \mathrm{g},$ what mass (in grams) of $\mathrm{Cr}_{2} \mathrm{O}_{3}$ is produced if the metal is converted completely to the oxide?

(c) What mass of $\mathrm{O}_{2}$ (in grams) is required for the reaction?

Chromium metal reacts with oxygen to give chromium(III) oxide, $\mathrm{Cr}_{2} \mathrm{O}_{3}$

(a) Write a balanced equation for the reaction.

(b) What mass (in grams) of $\mathrm{Cr}_{2} \mathrm{O}_{3}$ is produced if $0.175 \mathrm{g}$ of chromium metal is converted completely to the oxide?

(c) What mass of $\mathrm{O}_{2}$ (in grams) is required for the reaction?

Given the mass in grams of a substance in a reaction, calculate the mass in grams of another substance in the reaction.

Iron(III) oxide reacts with carbon to give iron and carbon monoxide.

$$

\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{C}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}(g)

$$

a. How many grams of C are required to react with $16.5 \mathrm{g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3} ?$

b. How many grams of CO are produced when $36.0 \mathrm{g}$ of C reacts?

c. How many grams of Fe can be produced when $6.00 \mathrm{g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3}$ reacts?

Iron(III) oxide reacts with carbon monoxide according to the equation:

Fe2O3(s) + 3 CO(g)-2 Fe(s) + 3 CO2(g)

A reaction mixture initially contains 22.55 g Fe2O3 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Chromium(III) oxide reacts with hydrogen sulfide (H2S) gas to form chromium(III) sulfide and water:

$$

\mathrm{Cr}_{2} \mathrm{O}_{3}(s)+3 \mathrm{H}_{2} \mathrm{S}(g) \longrightarrow \mathrm{Cr}_{2} \mathrm{S}_{3}(s)+3 \mathrm{H}_{2} \mathrm{O}(l)

$$

To produce 421 $\mathrm{g}$ of $\mathrm{Cr}_{2} \mathrm{S}_{3},$ how many (a) moles of $\mathrm{Cr}_{2} \mathrm{O}_{3}$ and (b) grams of $\mathrm{Cr}_{2} \mathrm{O}_{3}$ are required?

The balanced equation for a reaction in the process of reducing iron ore to the metal is

$$

\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{s})+3 \mathrm{CO}(\mathrm{g}) \longrightarrow 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_{2}(\mathrm{g})

$$

(a) What is the maximum mass of iron, in grams, that can be obtained from $454 \mathrm{g}(1.00 \mathrm{lb})$ of iron(III) oxide?

(b) What mass of $\mathrm{CO}$ is required to react with $454 \mathrm{g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3} ?$

The balanced equation for the reduction of iron ore to the metal using CO is $$\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{s})+3 \mathrm{CO}(\mathrm{g}) \rightarrow 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_{2}(\mathrm{g})$$

(a) What is the maximum mass of iron, in grams, that can be obtained from $454 \mathrm{g}(1.00 \mathrm{lb})$ of iron(III) Oxide?

(b) What mass of $\mathrm{CO}$ is required to react with $454 \mathrm{g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3} ?$