Question

A metallurgist reacts 320.0 grams of 75.0% by mass silver nitrate solution with an excess of copper metal. How many grams of silver metal can the metallurgist produce during the process?

Cu(s) + AgNO3 → Ag(s) + Cu(NO3)2

97.5 grams
125 grams
149 grams
152 grams

Answer 1

Answer:

= 152.40 g

Explanation:

The equation for the reaction is;

Cu(s) + AgNO3 → Ag(s) + Cu(NO3)2

Mass of silver nitrate = 320.0 g × 0.75

                                    =  240.0 g

Molar mass of silver nitrate =  169.87 g/mol

Therefore;

Moles of silver nitrate = 240.0 g/169.87 g/mol

                                    =  1.413 moles

Mole ratio of Silver nitrate to silver metal = 1 : 1

Therefore, moles of silver metal = 1.413 moles

Hence;

Mass of silver metal = 1.413 moles × 107.868 g/mol

                                 = 152.40 g