If 0.35 moles of silver nitrate eacts fully, how many moles of copper will react with it. cu + agno3 → cu(no3)2 + ag

Answer 1

Hello, Lota,

I know that Mike D. has already responded, but I noticed something with the equation as written. It isn't balanced. We need two (NO₃) groups on the right side, but only 1 group comes in from the left. We need a coefficient of 2 in front of the AgNO₃ . That also changes the Ag product on the right:

1Cu + 2AgNO₃ = 1Cu(NO₃)₂ + 2Ag

This changes the molar ratio of the Cu and AgNO₃ from what Mike D. had developed from the orginal equation. Now the equation says we need twice as much silver nitrate as copper. So if we used the entire 0..35 moles of silver nitrate, it would consume (1/2)(0.35 mole)= 0.175 moles of Cu. That would be 0.18 moles with 2 sig figs.

Bob

Answer 2

Well from the equation, as we have an invisible one before both the copper and the silver nitrate, we need the same number of moles of both to react together

so 0.35 moles of copper is required