Answer
Explanation
Given that:
The mass of pure silver needed = 800 g
Mass of zinc = 300 g
Mass of silver nitrate = 600 g
What to find:
Will the mass of zinc and silver nitrate be able to make 800 g of pure silver.
Step-by-step solution:
Step 1: Write the balanced equation for the reaction.
Zn + 2AgNO₃ → 2Ag + Zn(NO₃)₂
Step 2: Determine the moles of the reactants.
Using the mole formula, the moles of the reactants will be:
[tex]\begin{gathered} Moles\text{ }of\text{ }Zn=\frac{Mass}{Molar\text{ }mass}=\frac{300g}{65.38g\text{/}mol}=4.5886\text{ }mol \\ \\ Moles\text{ }of\text{ }AgNO_3=\frac{600g}{169.87g\text{/}mol}=3.5321\text{ }mol \end{gathered}[/tex]Step 3: Determine the moles of pure silver produced.
Using the mole ratio of Zn to AgNO₃ in the equation and the moles in step 2, we
