A metallurgist reacts 260.0 grams of 80.0% by mass silver nitrate solution with an excess of copper metal.
How many grams of silver metal can the metallurgist produce during the process? (1 point)
Cu(s) + AgNO3 → Ag(s) + Cu(NO3)2
A.108 grams
B.132 grams
C.146 grams
D.168 grams

132 g

Explanation:

Given data:

Mass of silver nitrate react = 260 g/100×80 = 208 g

Mass of silver metal produced = ?

Solution:

Chemical equation:

Cu + 2AgNO₃  →  2Ag + Cu(NO₃)₂

Number of moles of AgNO₃:

Number of moles = mass/molar mass

Number of moles = 208 g/ 169.87 g/mol

Number of moles = 1.22 mol

Now we will compare the moles of silver with solver nitrate from balance chemical equation.

            AgNO₃       :            Ag

                 2           :              2

                1.22        ;         1.22

Mass of Ag:

Mass = number of moles × molar mass

Mass = 1.22 mol × 107.8682 g/mol

Mass = 132 g