Question

Consider the process.
2C+02 - 2CO
Fe2O3+3CO - 2Fe + 3CO2
The volume of O2 required at STP which can produce sufficient CO to reduce 1 g Fe2O3 (Molar mass of Fe2O3 - 160 gm/mol) is
(1) 210 ml
(2) 180 ml
(3) 240 ml
(4) 160 ml​

Answer 1

Answer:

I think. 240 is a answer.....

Answer 2

The volume of oxygen gas required at STP is 210 mL

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of iron (III) oxide = 1 g

Molar mass of iron (III) oxide = 160 g/mol

Putting values in above equation, we get:

$\text{Moles of iron (III) oxide}=\frac{1g}{160g/mol}=6.25\times 10^{-3}mol$

For the given chemical reactions:

$2C+O_2\rightarrow 2CO$     .....(1)

$Fe_2O_3+3CO\rightarrow 2Fe+3CO_2$      ......(2)

By Stoichiometry of the reaction 2:

1 mole of iron (III) oxide reacts with 3 moles of CO

So, $6.25\times 10^{-3}$ moles of iron (III) oxide will react with = $\frac{3}{1}\times 6.25\times 10^{-3}=1.875\times 10^{-2}mol$ of CO

By Stoichiometry of the reaction 1:

2 moles of CO are produced by 1 mole of oxygen gas

So, $1.875\times 10^{-2}mol$ of Co will be produced by $\frac{1}{2}\times 1.875\times 10^{-2}=9.375\times 10^{-3}mol$ of oxygen gas

At STP:

1 mole of a gas occupies 22.4 L of volume

So, $9.375\times 10^{-3}mol$ of oxygen gas will occupy = $\frac{22.4}{1}\times 9.375\times 10^{-3}=0.210L=210mL$ of volume

Learn more about number of moles and volume at STP:

https://brainly.com/question/14090111

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