Question

a chemical company makes a silver by reacting silver nitrate would see the company needs to make 800 g of pure silver for a client they have 300 g of zinc and 600 g of silver nitrate will they be able to make enough silver to fill the order

Answer 1

Step-by-step 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:

`\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}`

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