Copper reacts with silver nitrate according to the equation: Cu(s) + 2AgNO3(aq)= Cu(NO3)2(ag) +2Ag(s). If 0.50mol of copper is added to 1.5mol of silver nitrate , which is the limiting reagent and how many moles of silver are formed
To determine the limiting reagent and the number of moles of silver formed, we need to compare the moles of copper and the moles of silver nitrate.
First, let's calculate the moles of copper (Cu):
Given: 0.50 mol Cu
Next, let's calculate the moles of silver nitrate (AgNO3):
Given: 1.5 mol AgNO3
From the balanced chemical equation, we can see that the ratio of Cu to AgNO3 is 1:2. This means that for every 1 mole of Cu, we need 2 moles of AgNO3.
To find out which reactant is the limiting reagent, we compare the ratio of moles of Cu to moles of AgNO3 using the stoichiometry.
Moles of Cu to moles of AgNO3 ratio:
1 mol Cu : 2 mol AgNO3
Now, let's calculate the moles of AgNO3 required for the reaction using the ratio above:
Moles of AgNO3 = (0.50 mol Cu) × (2 mol AgNO3 / 1 mol Cu) = 1.0 mol AgNO3
Since we have 1.5 mol of AgNO3 available, which is greater than the required amount of 1.0 mol, we can conclude that the silver nitrate (AgNO3) is in excess, and copper (Cu) is the limiting reagent in this reaction.
To find the number of moles of silver (Ag) formed, we use the stoichiometry and the balanced equation.
From the balanced equation, we can see that the ratio of moles of copper (Cu) to moles of silver (Ag) is 1:2. This means that for every 1 mole of Cu reacted, 2 moles of Ag are formed.
Using the limiting reactant (Cu), let's calculate the moles of silver formed:
Moles of Ag = (0.50 mol Cu) × (2 mol Ag / 1 mol Cu) = 1.0 mol Ag
Therefore, when 0.50 mol of copper is added to 1.5 mol of silver nitrate, copper is the limiting reagent, and 1.0 mol of silver is formed.