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. @taramgrant0543664 @photon336
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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katieb
  • katieb
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anonymous
  • anonymous
xCu + 2xAgNO3 --> xCu(NO3)2 + 2xAg If 2X=6.3, find X and hence no of moles reacted nd unreacted
anonymous
  • anonymous
Huh?
anonymous
  • anonymous
Here AgNO3 is the limiting reagent, so you have to calculate based on it

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anonymous
  • anonymous
Can you walk me through this whole equation because it's so confusing
anonymous
  • anonymous
The balanced eqn says that 1 mole of Cu requires 2 moles of AgNO3 to react with it. Since, you have 4.2 moles of Cu metal, it means you require 8.4 moles of AgNO3, which you don't have. So, you have to consider that you have 6.3 moles of AgNO3 that reacts with 6.3/2 moles(=3.15 moles) of Cu. So, no of moles of Ag formed=6.3 moles and, no of moles of unreacted Cu=4.2-3.15=1.05 moles
anonymous
  • anonymous
Whats the balanced equation?
anonymous
  • anonymous
Cu + 2AgNO3 --> Cu(NO3)2 + 2Ag
anonymous
  • anonymous
Ok then what?
anonymous
  • anonymous
The balanced eqn says that 1 mole of Cu requires 2 moles of AgNO3 to react with it. Since, you have 4.2 moles of Cu metal, it means you require 8.4 moles of AgNO3, which you don't have. So, you have to consider that you have 6.3 moles of AgNO3 that reacts with 6.3/2 moles(=3.15 moles) of Cu. So, no of moles of Ag formed=6.3 moles and, no of moles of unreacted Cu=4.2-3.15=1.05 moles
Kash_TheSmartGuy
  • Kash_TheSmartGuy

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