Determine the number of moles of silver produced from a solution of silver nitrate by one mole of copper

calculate the number of moles of copper which reacted
the number of moles of silver produced
the number of moles of silver which would have been produced by the reaction of one mole of copper with the silver nitrate solution

We had to put a coil in silver nitrate solution. the weight of the coil was 2.32 g

a the clean beaker of 125 ml weighed 86.45

We had to pour 25 ml of 0.2 M silver nitrate solution

We left the wire in the solution over night and saw that it had become furry and mouldly looking

when we weighed the coil it was 2.2 g

why did the wire change its weight?

why did the solution change colour? it was turqoise-blue

How does this compare with the number of moles predicted from the balanced chemical equation for the reaction?

In your experiment how many atoms of silver were produced?

1. copper metal was oxidized and went int solution as copper(II) ions
2. The copper ion caused the solution to go from colorless to blue.
3. ? mole Cu = 0.12 g / 63.5 g Cu/mole = 0.020 mole Cu
? mole Ag = 0.20 mole Ag/L x 0.025L = 0.050 mole Ag
ratio Ag/Cu = 0.050/0.020 = 2.5:1
equarion ratio 2:1 : Cu(s) + 2 Ag+(aq) ----------> 2 Ag(s) + Cu++(aq)
4. 0.020 mol Cu x 2 mol Ag/mol Cu x 6.02x10E23 atoms/mole = 2.4x10E22 Ag atoms.