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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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A chemist forms 16.6 g of potassium iodide by combining 3.9 g of potassium with 12.7 g of iodine. Show that these results are co
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Electronic configuration : It is defined as the representation of electrons around the nucleus of an atom.

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Paramagnetic compounds : They have unpaired electrons.

Diamagnetic compounds : They have no unpaired electrons that means all are paired.

The given electron configurations of Palladium are:

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(b) [Kr] 4d¹⁰

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(c) [Kr] 5s¹4d⁹

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