If 3.00 moles of NaCl were mixed with 0.2 L of 1.5 M of AgNO3, how many moles of solid would form? Include the formula for the solid.
AgNO3 + NaCl ==> AgCl(s) + NaNO3
You start with 3.0 mols NaCl. Add
200 mL x 1.5M AgNO3 = 0.300 mols.
You will form 0.3 mols AgCl. You will have 2.7 mols NaCl unreacted.
To determine the number of moles of solid that would form when NaCl reacts with AgNO3, we need to identify the balanced chemical equation for the reaction between NaCl and AgNO3.
The balanced chemical equation for the reaction is:
NaCl + AgNO3 -> AgCl + NaNO3
From the balanced equation, we can see that 1 mole of NaCl reacts with 1 mole of AgNO3 to form 1 mole of AgCl.
Given that 3.00 moles of NaCl were mixed with 0.2 L of 1.5 M AgNO3, we need to convert the volume of AgNO3 solution into the moles of AgNO3 using the molarity.
Molarity (M) = Moles (mol) / Volume (L)
Rearranging the equation, we get:
Moles (mol) = Molarity (M) * Volume (L)
Moles of AgNO3 = 1.5 M * 0.2 L = 0.3 moles
Since the stoichiometry of the reaction is 1:1 between NaCl and AgNO3, the moles of AgCl formed will also be 0.3 moles.
Therefore, when 3.00 moles of NaCl are mixed with 0.2 L of 1.5 M AgNO3, 0.3 moles of AgCl solid would form.
The formula for the solid formed is AgCl, which represents silver chloride.