I did not understand this question at all. Can anyone help by explaining it in detail. Thanx!Carbon (ii) oxide can be purified of oxygen impurities by having it react with cobalt (ii) oxide. If...

I did not understand this question at all. Can anyone help by explaining it in detail. Thanx!

Carbon (ii) oxide can be purified of oxygen impurities by having it react with cobalt (ii) oxide. If impure carbon oxide contains a volume of 1.5% oxygen, and reacts with cobalt (ii) oxide at 250 °C and 500 kPa, what mass of cobalt (ii) oxide will be required to purify 1.00 x 105L of carbon oxide?

4CoO + O2 = 2Co2O3

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Carbon (II) oxide reacts with oxygen easily to form carbon (IV) oxide. That is the reason for the removal of oxygen impurities by reacting it with cobalt (II) oxide to produce cobalt (III) oxide according to the given equation. Assuming room temperature conditions, the volume of oxygen in impure carbon (II) oxide is 1.5/100*105 L= 1.575L at 25 degrees C

At STP this should become 1.575*273/298 = 1.443L

In terms of moles this becomes = 1.443/22.4=0.06442 moles

According to the reaction, 4CoO + O2 -> 2Co2O3

1 mole O2 reacts with 4 moles of CoO. Hence in total,

 0.06442*4=0.25768 moles, or 0.25768*74.93g = 19.31g of CoO will be required to react with it completely.

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