CHEMISTRY STOICHIOMETRY

Question

A (1.5000x10^1) g piece of copper reacts with (1.34x10^2) g of silver nitrate dissolved in solution. What mass of silver will be formed from this reaction?

Note: Your answer is assumed to be reduced to the highest power possible.

Answer 1

To find the mass of Silver formed from this reaction you write the balanced equation.

2AgNO_3(aq) + Cu_(s)-------------->2 Ag_(S) + Cu(NO₃)_(aq)

You then find the moles of Ag and Cu present from the mass given.

15g of Copper/63.546gmol^-1 =0.236 moles of copper

134g of AgNO₃/169.873gmol^-1 =0.789 moles of AgNO₃

Using the mole ratio , you see that 2 moles of AgNO₃ reacts with one mole of Cu. Therefore 0.236 moles of Cu will react with 0.472 moles of AgNO_3.

To find the mass of silver formed your multiply moles of Ag with its RMM: 0.472moles*107.868= 50.91 grams of Ag.