(a) In a gaseous sample of oxygen atoms and diatomic oxygen in equilibrium at 298K andunder a pressure of 1atm, what fraction of
it is dissociated?
(b) At what temperature is the sample 1% dissociated?
(c) At 298K and under a pressure of 10,000 atm, what fraction is dissociated?
(b) At what temperature is the sample 1% dissociated?
(c) At 298K and under a pressure of 10,000 atm, what fraction is dissociated?
1 answer:
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The question is incomplete, here is the complete question:
When silver nitrate reacts with copper, copper(II) nitrate and silver are produced. The balanced equation for this reaction is:
Suppose 6 moles of silver nitrate react. The reaction consumes___ moles of copper. The reaction produces __ moles of copper(II) nitrate and __ moles of silver.
<u>Answer:</u> The amount of copper metal reacted is 3 moles, amount of copper (II) nitrate produced is 3 moles and amount of silver metal produced is 6 moles.
<u>Explanation:</u>
We are given:
Moles of silver nitrate = 6 moles
For the given chemical reaction:
- <u>For copper metal:</u>
By Stoichiometry of the reaction:
2 moles of silver nitrate reacts with 1 mole of copper metal
So, 6 moles of silver nitrate will react with = of copper metal
Moles of copper reacted = 3 moles
- <u>For copper(II) nitrate:</u>
By Stoichiometry of the reaction:
2 moles of silver nitrate produces 1 mole of copper(II) nitrate
So, 6 moles of silver nitrate will produce = of copper(II) nitrate
Moles of copper(II) nitrate produced = 3 moles
- <u>For silver metal:</u>
By Stoichiometry of the reaction:
2 moles of silver nitrate produces 2 moles of silver metal
So, 6 moles of silver nitrate will produce = of silver metal
Moles of silver metal produced = 3 moles
Hence, the amount of copper metal reacted is 3 moles, amount of copper (II) nitrate produced is 3 moles and amount of silver metal produced is 6 moles.