a 5.95 g sample of AgNO3 is reacted with excess BaCl2 according to the equation 2AgNO3 + BaCl2 yields 2AgCl + Ba(NO3)2 to give 3.17 g of AgCl. What is the percent yield of AgCl?
63.1506
To determine the percent yield of AgCl, we need to compare the actual yield of AgCl obtained in the reaction with the theoretical yield of AgCl that we can calculate based on the given information.
First, let's calculate the theoretical yield of AgCl using stoichiometry:
1) Calculate the molar mass of AgCl:
Ag: 107.87 g/mol
Cl: 35.45 g/mol
AgCl: 107.87 + 35.45 = 143.32 g/mol
2) Convert the mass of AgCl obtained (3.17 g) to moles:
Moles of AgCl = mass of AgCl / molar mass of AgCl
Moles of AgCl = 3.17 g / 143.32 g/mol ≈ 0.0221 mol
3) Based on the balanced equation, the mole ratio between AgNO3 and AgCl is 2:2. Therefore, the mole ratio between AgCl and AgNO3 is 1:1.
Since 2 moles of AgNO3 react to form 2 moles of AgCl, the theoretical yield of AgCl can be calculated:
Theoretical yield of AgCl = Moles of AgCl
So, the theoretical yield of AgCl is approximately 0.0221 mol.
Now, let's calculate the percent yield:
Percent yield = (Actual yield / Theoretical yield) × 100
Given that the actual yield of AgCl is 3.17 g and the theoretical yield is 0.0221 mol, we need to convert the theoretical yield back to grams.
4) Convert the theoretical yield of AgCl into grams:
Theoretical yield (grams) = Theoretical yield (moles) × molar mass of AgCl
Theoretical yield (grams) = 0.0221 mol × 143.32 g/mol ≈ 3.167 g
Now we can calculate the percent yield:
Percent yield = (3.17 g / 3.167 g) × 100 ≈ 100.09%
Therefore, the percent yield of AgCl is approximately 100.09%.
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in a particular experiment to prepare a compound, the theoritical yield is 34.7 g. if the actual yield is 31. 2 g, what is the percentage yield?
2AgNO3 + BaCl2 ==> 2AgCl + Ba(NO3)2
mols AgNO3 = grams/molar mass
Using the coefficients in the balanced equation, convert mols AgNO3 to mols
AgCl.
g AgCl = mols AgCl x molar mass
AgCl = ?. This is the theoretical yield; i.e., the yield if it were 100%.
Then % yield = (3.17/theoret yield)*100 = ?