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2 years ago

Zinc Sulfide reacts with oxygen according to the reaction:

Chemistry

1 answer:

zhuklara [117]2 years ago

6 0

The amount in moles of the excess reactant left is 0.5 mole

<h3>Balanced equation</h3>

2ZnS (s) + 3O₂(g) --> 2ZnO (s) + 2SO₂(g)

From the balanced equation,

2 moles of ZnS reacted with 3 moles of O₂

<h3>How to determine the excess reactant</h3>

From the balanced equation,

2 moles of ZnS reacted with 3 moles of O₂

Therefore,

4.2 moles of ZnS will react with =(4.2 × 3) / 2 = 6.3 moles of O₂

From the calculations made above, we can see that only 6.3 moles of O₂ out of 6.8 moles given, is required to react completely with 4.2 moles of ZnS.

Thus, ZnS is the limiting reactant and O₂ is the excess reactant.

<h3> How to determine the mole of the excess reactant remaining</h3>

The excess reactant is O₂. Thus the mole remaining after the reaction can be obtained as illustrated below:

Mole of O₂ given = 6.8 moles
Mole of O₂ that reacted = 6.3 moles
Mole of O₂ remaining =?

Mole of O₂ remaining = (Mole of O₂ given) - (Mole of O₂ that reacted)

Mole of O₂ remaining = 6.8 - 6.3

Mole of O₂ remaining = 0.5 mole

Learn more about stoichiometry:

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2 years ago

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3 years ago

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Answer:

Here's what I get.

Explanation:

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They are similar, except for the numbering of the valence shell orbitals.

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The ground state electron configuration of KrF is

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