Taking into account the reaction stoichiometry, 8 moles of Ag can be produced from 8 moles of AgNO₃ and 5 moles of Zn.
Reaction stoichiometry
In first place, the balanced reaction is:
2 AgNO₃ + Zn → 2 Ag + Zn(NO₃)₂
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- AgNO₃: 2 moles
- Zn: 1 mole
- Ag: 2 moles
- Zn(NO₃)₂: 1 mole
Limiting reagent
The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.
Limiting reagent in this case
To determine the limiting reagent, it is possible to use a simple rule of three as follows: if by stoichiometry 1 mole of Zn reacts with 2 moles of AgNO₃, 5 moles of Zn reacts with how many moles of AgNO₃?
[tex]amount of moles of AgNO_{3}= \frac{5 moles of Znx2 moles of AgNO_{3}}{1 mole of Zn}[/tex]
amount of moles of AgNO₃= 10 moles
But 10 moles of AgNO₃ are not available, 8 moles are available. Since you have less moles than you need to react with 5 moles of Zn, AgNO₃ will be the limiting reagent.
Moles of Ag formed
Considering the limiting reagent, the following rule of three can be applied: if by reaction stoichiometry 2 moles of AgNO₃ form 2 moles of Ag, 8 moles of AgNO₃ form how many moles of Ag?
[tex]amount of moles of Ag=\frac{8 moles of AgNO_{3}x2 moles of Ag }{2 moles of AgNO_{3}}[/tex]
amount of moles of Ag= 8 moles
Then, 8 moles of Ag can be produced from 8 moles of AgNO₃ and 5 moles of Zn.
Learn more about the reaction stoichiometry:
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