Chapter 12.3, Problem 31SP

Interpretation Introduction

Interpretation: The theoretical yield of silver in the given reaction is to be stated.

Concept Introduction: According to the law of conservation of mass, the mass can neither be created nor be destroyed. Every reaction must be balanced. With the help of the balanced equation, the limiting reagent can be found and in accordance with it, the amount of product can be calculated.

Answer to Problem 31SP

The theoretical yield of silver is 17.0 g.

Explanation of Solution

Given:

• 5.00 g of copper
• Excess silver nitrate

The reaction is given as follows:

  $\text{Cu}+2{\text{AgNO}}_{\text{3}}\to \text{Cu}{\left({\text{NO}}_3\right)}_2+2\text{Ag}$

The mol of copper is calculated as:

  $\begin{array}{c}\text{Mole}=\frac{\text{Mass}}{\text{Molar}\text{mass}}\\ =\frac{5.00\text{g}}{63.546\text{g/mol}}\\ =0.0787\text{mol}\end{array}$

According to the balanced equation,

  $\begin{array}{c}\text{1}\text{mol}\text{of}\text{Cu}\to 2\text{mol}\text{of}\text{Ag}\\ \text{0}\text{.0787}\text{mol}\text{of}\text{Cu}\to 2\times \text{0}\text{.0787}\text{mol}\text{of}\text{Ag}\\ \to 0.1574\text{mol}\text{of}\text{Ag}\end{array}$

The mass of copper is calculated as:

  $\begin{array}{c}\text{Mass}=\text{Mole}\times \text{Molar}\text{mass}\\ =0.1574\text{mol}\times 107.868\text{g/mol}\\ =\text{17}\text{.0}\text{g}\end{array}$

The theoretical yield of silver is 17.0 g.