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anonymous

  • one year ago

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

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  1. anonymous
    • one year ago
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    xCu + 2xAgNO3 --> xCu(NO3)2 + 2xAg If 2X=6.3, find X and hence no of moles reacted nd unreacted

  2. anonymous
    • one year ago
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    Huh?

  3. anonymous
    • one year ago
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    Here AgNO3 is the limiting reagent, so you have to calculate based on it

  4. anonymous
    • one year ago
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    Can you walk me through this whole equation because it's so confusing

  5. anonymous
    • one year ago
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    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

  6. anonymous
    • one year ago
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    Whats the balanced equation?

  7. anonymous
    • one year ago
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    Cu + 2AgNO3 --> Cu(NO3)2 + 2Ag

  8. anonymous
    • one year ago
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    Ok then what?

  9. anonymous
    • one year ago
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    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

  10. Kash_TheSmartGuy
    • one year ago
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    This link will help you - http://openstudy.com/study#/updates/53c1c134e4b00f624a91b3df

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