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

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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

Chemistry
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Start by balancing the equation Cu+ 2AgNO3 --> Cu(NO3)2 + 2Ag
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Do you know how to determine the limiting reactant?

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no
Why are both of them in Ag?
Ok so the limiting one would be the silver nitrate
That's it?? That seemed kind of easy...I think...
So to see how many silver nitrate was formed I would add 8.4 and 6.3?
I'm so confused right now?
Srry no question mark I am confused
Alright imma restart this then try to make it clearer.
ok
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.
I don't get it nvm just for get it
Sorry I cant think of how to explain it very well...
Its ok. Its just chem..

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