If 4.2 moles of copper metal reacts with 6.3 moles of silver nitrate, how many moles of silver metal can be formed, and how many moles of the excess reactant will be left over when the reaction is complete?

Unbalanced equation: Cu + AgNO3 → Cu(NO3)2 + Ag

Be sure to show all of your work.

@photon336 @welshfella @mathmate

Question

If 4.2 moles of copper metal reacts with 6.3 moles of silver nitrate, how many moles of silver metal can be formed, and how many moles of the excess reactant will be left over when the reaction is complete? 

Unbalanced equation: Cu + AgNO3 → Cu(NO3)2 + Ag

Be sure to show all of your work.

@photon336 @welshfella @mathmate

sweetburger · Answer

Start by balancing the equation Cu+ 2AgNO3 --> Cu(NO3)2 + 2Ag

anonymous · Answer

ok

sweetburger · Answer

Do you know how to determine the limiting reactant?

anonymous · Answer

no

anonymous · Answer

Why are both of them in Ag?

anonymous · Answer

Ok so the limiting one would be the silver nitrate

anonymous · Answer

That's it?? That seemed kind of easy...I think...

anonymous · Answer

So to see how many silver nitrate was formed I would add 8.4 and 6.3?

anonymous · Answer

I'm so confused right now?

anonymous · Answer

Srry no question mark I am confused

sweetburger · Answer

Alright imma restart this then try to make it clearer.

anonymous · Answer

ok

sweetburger · Answer

There is a 1:2 ratio between our Cu and AgNO3. If we have 4.2moles AgNO3 its a 2:1 ratio so 8.4moles. We only have 6.3moles of Cu though so 6:3:8.4 isnt 1:2 so 6.3moles is our limiting reagent and 6.3moles of product are formed so we need to find what is 1/2 of 6.3moles and that is 3.15moles so we had 3.15moles of  Cu react. So we initiall had 4.2moles of Cu so 4.2-3.15 = 1.05 which is also 2.1*.5. So the amount of Cu left over is 1.05moles.

anonymous · Answer

I don't get it nvm just for get it

sweetburger · Answer

Sorry I cant think of how to explain it very well...

anonymous · Answer

Its ok. Its just chem..