When 5.00 g of copper reacts with excess silver nitrate, silver metal and copper nitrate are...

Question:

When 5.00 g of copper reacts with excess silver nitrate, silver metal and copper nitrate are produced. What is the theoretical yield of silver in this reaction?

Stoichiometry:

The area of study in chemistry which is concerned with the quantities of chemical substances produced and required in a chemical reaction. The stoichiometric coefficients of the balanced chemical equation allow the determination of the products produced or reactants required.

Answer and Explanation:

As with all calculations in stoichiometry, we must establish the balanced chemical equation for the reaction.

{eq}Cu(s)~+~2~AgNO_3(aq)~\to~2~Ag(s)~+~Cu(NO_3)_2(aq) {/eq}

We can determine the theoretical yield using the molar mass of copper, silver and the stoichiometric coefficients from the balanced chemical equation.

{eq}5.00~g~Cu\times\frac{1~mol~Cu}{63.54~g}\times\frac{2~mol~Ag}{1~mol~Cu}\times\frac{107.8~g}{1~mol~Ag}~=~17.0~g~Ag {/eq}

Therefore, the theoretical yield of Ag is 17.0 g.


Learn more about this topic:

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Mass-to-Mass Stoichiometric Calculations

from Chemistry 101: General Chemistry

Chapter 9 / Lesson 3
55K

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