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Some Basic Concepts of Chemistry question

2022 · 29 Jun · Shift 1 · Q1

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Some Basic Concepts of Chemistry
2022 · 29 Jun · Shift 1 · Q1

Some Basic Concepts of Chemistry question

2022 · 29 Jun · Shift 1 · Q1

JEE MainChemistrySome Basic Concepts of ChemistryMCQ+4 / −1

Production of iron in blast furnace follows the following equation

Fe_3O_4

(s) + 4

CO

(g)

\to

3

Fe

(l) + 4

CO_2

(g) when 4.640 kg of

Fe_3O_4

and 2.520 kg of

CO

are allowed to react then the amount of iron (in g) produced is : [Given : Molar Atomic mass (g mol

-

1) : Fe = 56, Molar Atomic mass (g mol

-

1) : O = 16, Molar Atomic mass (g mol

-

1) : C = 12]

A
1400
B
2200
C
3360
D
4200

View written solutionFree

Correct answer: C

Write the balanced reaction

$Fe_3O_4 + 4CO \rightarrow 3Fe + 4CO_2$

Calculate molar masses

For $Fe_3O_4$ : $M(Fe_3O_4)=3(56)+4(16)=168+64=232\,g\,mol^{-1}$
For $CO$ : $M(CO)=12+16=28\,g\,mol^{-1}$

Convert given masses into moles

Moles of $Fe_3O_4$ : $n(Fe_3O_4)=\frac{4640}{232}=20\,mol$
Moles of $CO$ : $n(CO)=\frac{2520}{28}=90\,mol$

Find the limiting reagent

From the equation: $1\,mol\,Fe_3O_4 \text{ requires } 4\,mol\,CO$

So, for $20$ mol $Fe_3O_4$ , required $CO$ is: $20\times 4 = 80\,mol$

Available $CO = 90$ mol, which is excess.

Hence, $Fe_3O_4$ is the limiting reagent.

Calculate moles of iron produced

From the reaction: $1\,mol\,Fe_3O_4 \rightarrow 3\,mol\,Fe$

Thus, $20\,mol\,Fe_3O_4 \rightarrow 20\times 3 = 60\,mol\,Fe$

Convert moles of iron into mass

$m(Fe)=60\times 56 = 3360\,g$

Final answer

Amount of iron produced is: $\boxed{3360\,g}$

So, the correct option is C.

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