If you combine AgNO3 and Cu, what will be the products? Will it be Cu(NO3)2 and Ag? or CuNO3 and Ag?

Question

We had a quiz on Calorimetry, I wasn't sure if my balanced equation was correct. My balanced equation was 2AgNO3 + Cu -> Cu(NO3)2 + 2Ag. Is this correct? Or should I have written AgNO3+ Cu -> CuNO3 + Ag? PLS HELP ME!!! I realy do not know what oxidation no. of Cu to use (+1 or +2) I hope you guys can help me on this...

Answer 1

Okay, it's been a looooooong time since I had to use my chemistry skills, so lets see what I have:

Copper is more magnetic with electrons than silver is because it's electrons (with fewer of them) are close to the nucleus (or whatever you call it) of the element. Silver is more apt to lose its electrons with them being so far away.

Copper is more often found in a +2 state. So I'd say that's a safe bet to go with. I'd only assume a +1 state if your teacher said so.

So therefore: 2AgNO3 + Cu -> Cu(NO3)2 + 2 Ag would probably be your best bet.

But once again, it's been a long time since I used this so I don't know how right I might be.

Answer 2

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copper II is a plus two ion. when it is combined with nitrate a negative one ion, it takes two negative nitrates to equal the plus two of the copper. Cu(NO3)2 We must balance: Cu + AgNO3 = Cu(NO3)2 + Ag We need 2 NO3 on the left to balance the 2 on the right Cu + 2AgNO3 = Cu(NO3)2 + Ag and now we need to put a 2 in front of the Ag on the right

Answer 3

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RE:
If you combine AgNO3 and Cu, what will be the products? Will it be Cu(NO3)2 and Ag? or CuNO3 and Ag?
We had a quiz on Calorimetry, I wasn't sure if my balanced equation was correct. My balanced equation was 2AgNO3 + Cu -> Cu(NO3)2 + 2Ag. Is this correct? Or should I have written AgNO3+ Cu -> CuNO3 + Ag? PLS HELP ME!!! I realy do not know what oxidation no. of Cu to use (+1 or +2) I hope...

Answer 4

Agno3 Cu

Answer 5

Cu Agno3

Answer 6

Very good point...

Cu(+2) is more stable in water than Cu(+) so I think you should have Cu(+2). However I think, but could be wrong, that actually the standard potential of the reaction actually favours Cu(+)...

Nonetheless in several sites I saw the reaction giving Cu(+2).
Here is a nice one
http://jchemed.chem.wisc.edu/jcesoft/cca/CCA1/R1MAIN/CD1R1970.HTM

[Edit] I looked again at the standard potentials and actually the reaction to Cu(+2) is more favoured (E0 total reaction 0.458 Volt when Cu(+2) is produced vs 0.279 Volt for the case of Cu(+))

Answer 7

First, the equation is already balanced. To answer your question in you additional details: Copper(II) means that you have 1 Cu but it is a +2 charge. For example, Copper(III) means that the Cu has a +3 charge.

Answer 8

Silver is higher than copper on the electrochemical series, so in theory the copper metal would release its electrons to silver. However, their V0 values, being so close, means that the probability of the reaction actually occuring is quite low. Nonetheless:

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

1/2 Equations:
Cu(s) --> Cu2+(aq) + 2e
2Ag+(aq/l) + 2e --> 2Ag(s)

Answer 9

The valence of copper, is -2

NO3 is one.

So it would be Cu+ 2 NO3

Answer 10

This is a simple single replacement reaction, that's all it is. You will get:

AgNO3 + Cu -> CuNO3 + Ag (precipated)

Don't try to make things hard. It is a very simple formula, but you make it hard by assuming Cu+2 instead of Cu+1. And it really doesn't matter anyway, as it is the Ag precipitate that matters most.