How many moles of Ag can be produced if 350.g of Cu are reacted with excess AgNO3 according to the equation Cu(s) plus 2AgNO3(aq) plus Cu(NO3)2(aq)?
I am not certain I buy your equation as typed. However, one mole of copper will replace 2 moles of Silver in
Cu +2Ag(NO3) >> Cu(NO3)2 + 2Ag
Figure the moles of 350g copper, double that amount of moles, that will be the moles of silver.
We are looking for moles, it's not that complicated so don't make it sound complicated.
111.8922
To determine the number of moles of Ag that can be produced, we first need to determine the balanced chemical equation for the reaction:
Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s)
From the balanced equation, we can see that 1 mole of Cu reacts with 2 moles of AgNO3 to produce 2 moles of Ag. This means that the stoichiometric ratio for Ag to Cu is 2:1.
Now, we will calculate the number of moles of Cu using its given mass of 350 g. To do this, we'll need the molar mass of Cu, which is 63.55 g/mol.
Number of moles of Cu = Mass of Cu / Molar mass of Cu
Number of moles of Cu = 350 g / 63.55 g/mol
Number of moles of Cu = 5.5083 mol
Since AgNO3 is in excess, it means that Cu is the limiting reactant in this reaction. Therefore, the number of moles of Ag produced will be equal to half the number of moles of Cu (based on the stoichiometric ratio).
Number of moles of Ag = 0.5 * Number of moles of Cu
Number of moles of Ag = 0.5 * 5.5083 mol
Number of moles of Ag = 2.7541 mol
Thus, 2.7541 moles of Ag can be produced when 350 g of Cu reacts with excess AgNO3.