Can someone instruct me on how to go about balancing this redox equation?

Question

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

As many steps as you can give would be great! My book is the worst and I know nothing about where or how to begin!
Thanks so much!

Answer 1

In a redox problem, always determine the oxidation states of the oxidized atom and of the reduced atom.

Cu: 0 going to +2, a loss of 2 electrons (the oxidized atom)
Ag: +1 going to 0, a gain of 1 electron (the reduced atom)

Since the electron gained must equal the electrons lost, you need 2 Ag atoms for each Cu atom

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

Everything is balanced: electrons, Cu, Ag, and NO3-

Answer 2

I usualy do it by looking at it (I'm not certian if there is a specific mathmatical procedure)

Notice that silver (Ag) is reduced from +1 to 0 and copper (Cu) is oxidized from 0 to +2. (The nitrate group has a -1 charge).

So, 1 copper can reduce 2 silvers:

Cu + 2 Ag(NO3) .>> Cu(NO3)2 + 2 Ag

Answer 3

Not much of a redox equation. The result is
Cu+ 2 AgNO3 -> 2Ag + Cu(NO3)2

It does get messy when you have oxidizing agents like Cr2O7 and acids and bases.