Copper in Silver Nitrate Lab: Making Silver
Sabrina Kate S. Carranza – Chemistry Hour 6

I. Purpose:
The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.

II. Hypothesis: /3
-If the copper metal is submerged in the silver nitrate solution then in reaction, a pure, solid (Ag) silver product is created with an excess of (Cu (NO3)2) copper (II) aqueous liquid because a single displacement reaction occurs where the balance equation is then
2AgNO3 + Cu(s) 2Ag + Cu (NO3) 2

III. …show more content…

2AgNO3 + Cu(s) 2Ag + Cu(NO3) 2

2) Given that 50.00 mL of 0.50mL of AgNO3 contains 4.25 of AgNO3, calculate the theoretical yield of Ag that should be formed when 50.00mLof 0.50M AgNO3 reacts with an excess of Cu.

(4.25 g AgNO3 / 1) * (1 mol AgNO3/ 169.91 g AgNO3) * (2 mol Ag/2 mol AgNO3) * (107.91 g Ag/ 1 mol Ag) = 2.70 g Ag

3) Compare the theoretical yield of Ag with the experimental yield from your data table. Calculate the percent error.

Percent error= | Exp. – Theo. / Theo. | *100
| 2.607- 2.70 /2.70 | 0.035 *100 = 3.57%

4) Calculate the mass of copper required to react completely with 4.25 g of AgNO3

(4.25 g AgNO3 / 1) * (1 mol AgNO3/ 169.91 g AgNO3) * (1 mol Cu/2 mol AgNO3) * (63.54 g Ag/ 1 mol Cu) = 0.795 g Cu

5) Compare the mass of the copper hat you obtained in calculation #4 with the mass of copper that reacted in your experiment. Explain any differences.

Percent error= | Exp. – Theo. / Theo. | *100
| 0.7787 g – 0.795 g/ 0.795 g | *100 = 2.05%

VI. Conclusion:
Referring to my initial prediction, my data results are supported by my hypothesis where I stated –“If the copper metal is submerged in the silver nitrate