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

= 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