if 1.00 g of silver nitrate is combined with 1.00g of sodium chloride what is the mass of the solid if you have 75% yield?
First determine limiting reagent.
AgNO3 + NaCl ==> AgCl + NaNO3
mols AgNO3 = grams/molar mass
mols NaCl = grams/molar mass
Convert mols AgNO3 to mols AgCl using the coefficients in the balanced equation.
Do the same for NaCl.
It is likely these two values will not agree which means one of them is wrong. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent responsible for that number is the limiting reagent.
Using the smaller number, convert to grams AgCl. g AgCl = mols AgCl x molar mass AgCl. This is the theoretical yield; i.e., yield at 100%.
Theoretical yield x 0.75 = amount produced at 75% yield.
To calculate the mass of the solid formed when 1.00 g of silver nitrate is combined with 1.00 g of sodium chloride, we need to understand the chemical reaction that occurs between these two compounds.
The balanced chemical equation for the reaction between silver nitrate (AgNO3) and sodium chloride (NaCl) is:
AgNO3 + NaCl -> AgCl + NaNO3
From the balanced equation, we can see that silver nitrate reacts with sodium chloride to produce silver chloride and sodium nitrate.
Next, we need to calculate the amount of AgCl formed by considering the 75% yield.
1. Calculate the molar masses of the compounds involved:
- AgNO3 molar mass = 107.87 g/mol
- NaCl molar mass = 58.44 g/mol
- AgCl molar mass = 143.32 g/mol
2. Convert the mass of each reactant (AgNO3 and NaCl) to moles:
- Moles of AgNO3 = mass of AgNO3 (in grams) / molar mass of AgNO3
= 1.00 g / 107.87 g/mol ≈ 0.00926 mol
- Moles of NaCl = mass of NaCl (in grams) / molar mass of NaCl
= 1.00 g / 58.44 g/mol ≈ 0.01712 mol
3. Determine the limiting reactant:
The limiting reactant is the reactant that will be completely consumed in the reaction, thus determining the maximum amount of product that can be formed. To identify the limiting reactant, we compare the mole ratios of AgNO3 and NaCl in the balanced equation (1:1).
Since the molar ratio of AgNO3 to NaCl is 1:1, both reactants are in excess and will react completely.
4. Calculate the theoretical yield of AgCl:
Because both reactants are in excess and will react completely, the theoretical yield of AgCl will be equal to the total amount of reactants used.
The total amount of reactants used is the sum of the moles of AgNO3 and NaCl:
- Total moles of reactants = Moles of AgNO3 + Moles of NaCl
= 0.00926 mol + 0.01712 mol ≈ 0.02638 mol
5. Calculate the mass of AgCl using the theoretical yield:
- Mass of AgCl = moles of AgCl x molar mass of AgCl
= 0.02638 mol x 143.32 g/mol
≈ 3.78 g
6. Calculate the actual yield based on the given 75% yield:
- Actual yield = theoretical yield x yield percentage
= 3.78 g x 0.75
≈ 2.84 g
Therefore, if the yield is 75%, the mass of the solid formed will be approximately 2.84 grams.
To find the mass of the solid if you have a 75% yield, we first need to determine the limiting reagent in the reaction between silver nitrate (AgNO3) and sodium chloride (NaCl). The limiting reagent is the reactant that is entirely consumed and determines the maximum amount of product formed.
Let's calculate the moles of each reactant:
1. Convert the mass of silver nitrate to moles:
molar mass of AgNO3 = atomic mass of Ag + atomic mass of N + 3 * atomic mass of O
= (107.87 g/mol + 14.01 g/mol + 3 * 16.00 g/mol)
= 169.87 g/mol
moles of AgNO3 = mass of AgNO3 / molar mass of AgNO3
= 1.00 g / 169.87 g/mol
= 0.00588 mol (approximately)
2. Convert the mass of sodium chloride to moles:
molar mass of NaCl = atomic mass of Na + atomic mass of Cl
= 22.99 g/mol + 35.45 g/mol
= 58.44 g/mol
moles of NaCl = mass of NaCl / molar mass of NaCl
= 1.00 g / 58.44 g/mol
= 0.0171 mol (approximately)
Next, we compare the mole ratio between AgNO3 and NaCl:
1 mol AgNO3 reacts with 1 mol NaCl
As both reactants have a 1:1 ratio, the limiting reagent will be the one with fewer moles, which is silver nitrate (AgNO3) in this case.
Since the reaction has a 75% yield, only 75% of the limiting reagent will react to form the product. Therefore, we'll calculate the final mass of the solid (product) using this yield:
mass of solid = mass of limiting reagent * yield
mass of solid = 0.00588 mol * 169.87 g/mol * 0.75
= 0.746 g
So, the mass of the solid will be approximately 0.746 grams.