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olasank [31]
3 years ago
11

Dinitrogen tetraoxide partially decomposes according to the following equilibrium:

Chemistry
1 answer:
Bas_tet [7]3 years ago
5 0

Answer:

Keq for this reaction is 0.87 (option a.)

Explanation:

The equilibrium is this:

N₂O₄  ⇄ 2N₂O₂

1 mol of N₂O₄ decomposes to 2 moles N₂O₂

                    N₂O₄  ⇄ 2N₂O₂

Initially       0.04m           -

React               x             2x

Initially I have 0.04 moles of N₂O₄. Some amount (x) reacts to decompose and make 2 moles of N₂O₂; according to reaction, ratio is 1:2.

So if x amount of compound, reacted. I will have the double, as product decomposed.

                    N₂O₄  ⇄ 2N₂O₂

Initially       0.04m           -

React               x             2x

Eq.              0.055m       2x

We have moles of N₂O₄ in equilibrium, so we have to know how many amount has reacted.

(0.04 - 0.0055) = 0.0345

The double of this, is what we have in equilibrium of N₂O₂.

0.0345 .2 = 0.069

Let's make Kc:

[N₂O₂]² / [N₂O₄]

0.069² / 0.0055 = 0.87

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Answer:

<h2>1.8662 × 10²⁴ atoms</h2>

Explanation:

The number of atoms can be found by using the formula

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We have the final answer as

<h3>1.8662 × 10²⁴ atoms</h3>

Hope this helps you

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Answer:

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