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Sonja [21]
3 years ago
13

Find the mass of oxygen in grams produced by the decomposition of 100.0 g of CO2

Chemistry
1 answer:
SSSSS [86.1K]3 years ago
7 0

The balanced chemical equation is :

2CO_2->2CO+O_2\\\\

Moles of CO_2 ,

n = \dfrac{100\ g}{44.01\ g/mol}\\\\n=2.27\ mol

Now, by given chemical equation , we can see 2 mole of CO_2 react with 1 mole of O_2.

So , 2.27 mole react with :

N=\dfrac{2.27}{2}\ mol\\\\N=1.135\ mol

Mass of oxygen is :

M = N \times 16\\\\M=1.135\times 16\ g\\\\M =18.16\ g

Therefore, mass of oxygen in grams produced is 18.16 g.

Hence, this is the required solution.

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3 years ago
If 4000 g of Fe2O3 reacts, how many moles of CO are needed?<br> (add work)
7nadin3 [17]

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75.15 mol.

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It is clear that 1.0 mole of Fe₂O₃ reacts with 3.0 moles of CO to produce 2.0 moles of Fe and 3.0 moles of CO₂.

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  • we need to calculate the no. of moles of (4000 g) of Fe₂O₃:

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<u>Using cross multiplication:</u>

1.0 mole of Fe₂O₃ needs → 3.0 moles of CO,

∴ 25.05 mole of Fe₂O₃ needs → ??? moles of CO.

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3 years ago
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Answer:

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F-, a fluorine anion.

Explanation:

I got u

4 0
3 years ago
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