Question

Cu + 2AgNO3 → Cu(NO3)2 + 2Ag

If a 40. g sample of Copper is used with an excess of silver nitrate, calculate the theoretical yield of silver. What is the percent yield of the silver, if 120 g was collected?

Answer 1

`m_(Ag)=135.8gAg`

`Y=88.4\%`

Step-by-step explanation:

Hello there!

In this case, according to the described chemical reaction, it is possible to compute the theoretical mass of silver as mass via the 1:2 mole ratio of copper to silver and their atomic mass in the periodic table, in order to perform the following stoichiometric setup:

`m_(Ag)=40.gCu*(1molCu)/(63.55gCu)*(2molAg)/(1molCu)*(107.87gAg)/(1molAg)\\\\ m_(Ag)=135.8gAg`

Next, given the actual yield of 120 g, we compute the percent yield via:

`Y=(120g)/(135.8g)*100\%\\\\Y=88.4\%`

Regards!