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.

@taramgrant0543664 @photon336

Answer 1

xCu + 2xAgNO3 --> xCu(NO3)2 + 2xAg
If 2X=6.3, find X and hence no of moles reacted nd unreacted

Answer 2

Huh?

Answer 3

Here AgNO3 is the limiting reagent, so you have to calculate based on it

Answer 4

Can you walk me through this whole equation because it's so confusing

Answer 5

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

Answer 6

Whats the balanced equation?

Answer 7

Cu + 2AgNO3 --> Cu(NO3)2 + 2Ag

Answer 8

Ok then what?

Answer 9

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

Answer 10

This link will help you - http://openstudy.com/study#/updates/53c1c134e4b00f624a91b3df