what is the percentage yield of c2h2 with 50g of cac2 reacts with water to yield 13.5g of c2h2
CaC2 + 2H2O --> Ca(OH)2 + C2H2
mols CaC2 = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols CaC2 to mols C2H2
Then grams C2H2 = mols C2H2 x molar mass C2H2. This the theoretical yield (TY).
The actual yield (AY) is 13.5 grams.
%yield = (AY/TY)*100 = ?
65%
To calculate the percentage yield of C2H2 (acetylene) in this reaction, we need to compare the actual yield (13.5g) to the theoretical yield, which can be calculated using stoichiometry.
First, let's write the balanced chemical equation for the reaction:
CaC2 + 2H2O -> Ca(OH)2 + C2H2
From the equation, we can see that 1 mole of CaC2 reacts to produce 1 mole of C2H2. We can use the molar mass of CaC2 (64g/mol) to convert the given mass (50g) into moles:
molar mass of CaC2 = 64g/mol
moles of CaC2 = mass / molar mass = 50g / 64g/mol = 0.78 mol
According to the stoichiometry, 0.78 moles of CaC2 will yield an equal number of moles of C2H2. Therefore, the theoretical yield of C2H2 is also 0.78 moles.
To convert the moles of C2H2 back into grams, we can use the molar mass of C2H2 (26g/mol):
theoretical yield of C2H2 = moles of C2H2 * molar mass of C2H2 = 0.78 mol * 26g/mol = 20.28g
Now that we have the theoretical yield (20.28g) and the actual yield (13.5g), we can use the following equation to calculate the percentage yield:
percentage yield = (actual yield / theoretical yield) * 100
= (13.5g / 20.28g) * 100
= 66.57%
Therefore, the percentage yield of C2H2 in this reaction is approximately 66.57%.
To determine the percentage yield of C2H2, we need to compare the actual yield (the amount obtained in the experiment) with the theoretical yield (the maximum amount that can be produced based on stoichiometry). Here's how to calculate it step by step:
1. Write down the balanced chemical equation:
C2H2 + 2H2O → Ca(OH)2 + C2H2
2. Calculate the molar mass of calcium carbide (CaC2):
CaC2 = 40.08 g/mol (calcium) + 12.01 g/mol (carbon) = 52.09 g/mol
3. Convert the mass of CaC2 given (50g) into moles:
50g ÷ 64.09 g/mol = 0.779 mol CaC2
4. Determine the stoichiometric ratio between CaC2 and C2H2 from the balanced equation:
1 mol CaC2 produces 1 mol C2H2
5. Calculate the theoretical yield of C2H2 (in moles) based on the amount of CaC2 used:
0.779 mol C2H2
6. Convert the theoretical yield from moles to grams:
The molar mass of C2H2 is 26.04 g/mol.
0.779 mol C2H2 × 26.04 g/mol = 20.3 g C2H2
7. Calculate the percentage yield:
Actual yield: 13.5 g
Theoretical yield: 20.3 g
Percentage Yield = (Actual yield / Theoretical yield) × 100
Percentage Yield = (13.5 g / 20.3 g) × 100 = 66.50%
Therefore, the percentage yield of C2H2 in this reaction is 66.50%.