Copper metal (Cu) reacts with silver nitrate (AgNO3) in aqueous solution to form Ag and Cu (NO3) 2. An excess of AgNO3 is present. The balanced chemical equation is shown below.

Cu + 2AgNO3 - - - > Cu (NO3) 2 + 2Ag

The molar mass of Cu is 63.5 g/mol. The molar mass of Ag is 107.9 g/mol. What mass, in grams, of Ag is produced from reaction of 31.75 g of Cu?

26.95

107.9

215.91

431.82

Question

Todd Molina

Chemistry

11 November, 22:10

Copper metal (Cu) reacts with silver nitrate (AgNO3) in aqueous solution to form Ag and Cu (NO3) 2. An excess of AgNO3 is present. The balanced chemical equation is shown below.

Cu + 2AgNO3 - - - > Cu (NO3) 2 + 2Ag

The molar mass of Cu is 63.5 g/mol. The molar mass of Ag is 107.9 g/mol. What mass, in grams, of Ag is produced from reaction of 31.75 g of Cu?

26.95

107.9

215.91

431.82

+2

Answers (1)

Know the Answer?

Alfredo Mccarthy · Answer 1

we are given the reaction Cu + 2AgNO3 - - - > Cu (NO3) 2 + 2Ag. This means for every mole Cu used, there are 2 moles of Ag produced. In this case, given 31.75 g Cu, converting to moles through molar mass and using stoichiometric ratio and the molar mass of Ag, the mass Ag produced is 107.9 grams.