anonymous
  • anonymous
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
  • Stacey Warren - Expert brainly.com
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SOLVED
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chestercat
  • chestercat
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sweetburger
  • sweetburger
Start by balancing the equation Cu+ 2AgNO3 --> Cu(NO3)2 + 2Ag
anonymous
  • anonymous
ok
sweetburger
  • sweetburger
Do you know how to determine the limiting reactant?

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

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