How much AgCl will be formed by adding 200mL of 5N HCl to a solution containing 1.7g AgNO3?
This is a limiting reagent (LR) problem and you know that because amounts are given for BOTH reactants. I do these the long way---easier to exlpain for me.
AgNO3 + HCl ==> AgCl + HNO3
mols AgNO3 = grams/molar mass = ?
mols HCl = M x L = ?
Using the coefficients in the balanced equation, convert mols AgNO3 to mols of AgCl.
Do the same to convert mols HCl to mols AgCl.
It is likely that the two values will not be the same which means one of them is not right; the correct value in LR problems is ALWAYS the smaller value and the reagent responsible for producing that number is the LR.
Using the smaller value for mols AgCl, convert to grams. g = mols x molar mass.
To calculate the amount of AgCl formed, we need to use stoichiometry, which involves using balanced chemical equations to relate the reactants and products in a chemical reaction.
The balanced chemical equation for the reaction between AgNO3 and HCl is:
AgNO3 + HCl → AgCl + HNO3
From the balanced equation, we can see that 1 mole of AgNO3 reacts with 1 mole of HCl to form 1 mole of AgCl.
First, let's convert the given quantities to moles:
1 mole of AgNO3 = molar mass of AgNO3 = 107.87 g/mol
1 mole of HCl = molar mass of HCl = 36.46 g/mol
Mass of AgNO3 = 1.7 g
Moles of AgNO3 = 1.7 g / 107.87 g/mol ≈ 0.0158 mol
Next, we need to determine the number of moles of HCl present in the solution.
N is a measure of concentration, defined as the number of moles of solute per liter of solution. In this case, the given concentration is 5N. This means that 5 moles of HCl are present in 1 liter of solution.
Since we have 200 mL of 5N HCl, we can calculate the moles of HCl using the following conversion:
Volume of HCl = 200 mL = 200/1000 L = 0.2 L
Moles of HCl = concentration (N) × volume (L)
= 5N × 0.2 L
= 1 mol
Now, we compare the number of moles of AgNO3 and HCl to determine the limiting reagent. The limiting reagent is the reactant that is entirely consumed in the reaction and determines the amount of product formed.
From the balanced chemical equation, we see that 1 mole of AgNO3 reacts with 1 mole of HCl to form 1 mole of AgCl. Therefore, the moles of AgCl formed will be equal to the moles of the limiting reagent.
In this case, since 0.0158 mol of AgNO3 is less than 1 mol of HCl, AgNO3 is the limiting reagent.
So, the amount of AgCl formed will be equal to the moles of AgNO3:
Moles of AgCl formed = moles of AgNO3 = 0.0158 mol
Finally, we convert the moles of AgCl to grams using the molar mass of AgCl:
Molar mass of AgCl = 107.87 g/mol
Mass of AgCl formed = moles of AgCl × molar mass of AgCl
= 0.0158 mol × 143.32 g/mol (molar mass of AgCl)
= 2.25 g
Therefore, by adding 200 mL of 5N HCl to a solution containing 1.7 g AgNO3, 2.25 g of AgCl will be formed.
To find out how much AgCl will be formed, we need to identify the limiting reagent. The limiting reagent is the reactant that gets completely consumed and limits the amount of product that can be formed.
Let's calculate the number of moles of AgNO3 and HCl:
1. Moles of AgNO3:
- Given mass of AgNO3: 1.7g
- Molar mass of AgNO3: 107.87 g/mol
- Moles of AgNO3 = mass / molar mass
= 1.7g / 107.87 g/mol
= 0.0157 mol
2. Moles of HCl:
- Given volume of HCl: 200 mL
- Concentration of HCl: 5N (N refers to normality, which is the number of equivalents of solute present per liter of solution)
- Since N = molarity * number of equivalents, we need to calculate the molarity first.
- Molarity of HCl = 5N / eq
- eq for HCl = 1 (as HCl is a monoprotic acid)
- Molarity of HCl = 5N / 1 = 5M (M refers to molarity)
- Volume of HCl in liters = 200 mL / 1000 mL/L = 0.2 L
- Moles of HCl = Molarity * volume
= 5M * 0.2 L
= 1 mol
Now, let's identify the limiting reagent:
The balanced chemical equation for the reaction between AgNO3 and HCl is:
AgNO3 + HCl -> AgCl + HNO3
From the balanced equation, we can see that the stoichiometric ratio between AgNO3 and AgCl is 1:1.
The stoichiometric ratio between AgNO3 and HCl is also 1:1.
Comparing the moles of AgNO3 (0.0157 mol) and HCl (1.0 mol), we see that AgNO3 is the limiting reagent because it has less moles.
Now, let's calculate the amount of AgCl formed:
Since the stoichiometric ratio between AgNO3 and AgCl is 1:1, the moles of AgCl formed will be the same as the moles of AgNO3.
Therefore, the amount of AgCl formed is 0.0157 mol.
To calculate the mass of AgCl formed, we need to know the molar mass of AgCl:
Molar mass of AgCl = 107.87 g/mol (atomic mass of Ag) + 35.45 g/mol (atomic mass of Cl)
= 143.32 g/mol
Now, let's calculate the mass of AgCl formed:
Mass of AgCl = moles of AgCl * molar mass of AgCl
= 0.0157 mol * 143.32 g/mol
≈ 2.25 g
Therefore, approximately 2.25 grams of AgCl will be formed by adding 200 mL of 5N HCl to a solution containing 1.7g AgNO3.