Respuesta :
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:
[tex]2AgNO_3+Cu\rightarrow Cu(NO_3)_2+2Ag[/tex]
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.
Answer: 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.
Explanation:
We are given:
Moles of silver nitrate = 6 moles
For the given chemical reaction:
[tex]2AgNO_3+Cu\rightarrow Cu(NO_3)_2+2Ag[/tex]
- For copper metal:
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 = [tex]\frac{1}{2}\times 6=3mol[/tex] of copper metal
Moles of copper reacted = 3 moles
- For copper(II) nitrate:
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 = [tex]\frac{1}{2}\times 6=3mol[/tex] of copper(II) nitrate
Moles of copper(II) nitrate produced = 3 moles
- For silver metal:
By Stoichiometry of the reaction:
2 moles of silver nitrate produces 2 moles of silver metal
So, 6 moles of silver nitrate will produce = [tex]\frac{2}{2}\times 6=6mol[/tex] 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.
