Calculate the percent yield of Cl2(g) in the electrolytic decomposition of
hydrogen chloride if 25.8 g of HCl produces 13.6 g of chlorine gas.
To calculate the percent yield of Cl2(g) in the electrolytic decomposition of HCl, we need to compare the actual yield (the amount of Cl2 produced) to the theoretical yield (the maximum amount of Cl2 that could be produced).
1. Calculate the molar mass of HCl:
- Hydrogen (H) has a molar mass of 1.01 g/mol.
- Chlorine (Cl) has a molar mass of 35.45 g/mol.
Molar mass of HCl = 1.01 g/mol + 35.45 g/mol = 36.46 g/mol.
2. Convert the mass of HCl to moles:
Moles of HCl = mass of HCl / molar mass of HCl = 25.8 g / 36.46 g/mol = 0.708 mol.
3. Using the balanced chemical equation for the decomposition of HCl:
2 HCl(aq) → H2(g) + Cl2(g)
We can see that 2 moles of HCl produce 1 mole of Cl2, so the theoretical yield of Cl2 is half the moles of HCl.
Theoretical yield of Cl2 = 0.708 mol / 2 = 0.354 mol.
4. Convert the theoretical yield of Cl2 from moles to grams:
Mass of Cl2 = moles of Cl2 × molar mass of Cl2 = 0.354 mol × 70.90 g/mol = 25.06 g.
5. Calculate the percent yield:
Percent yield = (Actual yield / Theoretical yield) × 100
Percent yield = (13.6 g / 25.06 g) × 100 = 54.23%
Therefore, the percent yield of Cl2 in the electrolytic decomposition of HCl is approximately 54.23%.
To calculate the percent yield of Cl2(g) in the electrolytic decomposition of hydrogen chloride, we need to compare the actual yield (the amount of product obtained) with the theoretical yield (the maximum amount of product that could be obtained under ideal conditions).
The first step is to calculate the molar mass of HCl and Cl2.
The molar mass of HCl is the sum of the atomic masses of hydrogen (H) and chlorine (Cl):
HCl = 1.01 g/mol (atomic mass of H) + 35.45 g/mol (atomic mass of Cl) = 36.46 g/mol.
The molar mass of Cl2 is the sum of the atomic masses of chlorine (Cl) multiplied by 2 (since there are two chlorine atoms in one molecule of Cl2):
Cl2 = 35.45 g/mol (atomic mass of Cl) x 2 = 70.90 g/mol.
Next, we need to determine the theoretical yield of Cl2, which is the amount of Cl2 that should have been produced based on stoichiometry.
From the balanced chemical equation for the electrolytic decomposition of HCl:
2HCl -> Cl2 + H2,
we can see that for every 2 moles of HCl, 1 mole of Cl2 is produced. Therefore, we need to convert the given mass of HCl to moles and then calculate the moles of Cl2 produced.
Number of moles of HCl = mass / molar mass = 25.8 g / 36.46 g/mol = 0.7086 mol.
Since the stoichiometry indicates that for every 2 moles of HCl, 1 mole of Cl2 is produced, we can calculate the moles of Cl2 produced:
0.7086 mol HCl x (1 mol Cl2 / 2 mol HCl) = 0.3543 mol Cl2.
Finally, we can calculate the percent yield using the formula:
percent yield = (actual yield / theoretical yield) x 100%.
Actual yield = 13.6 g of Cl2 (given).
Percent yield = (13.6 g / 0.3543 mol) x 100% = 3840%.
Therefore, the percent yield of Cl2 in the electrolytic decomposition of hydrogen chloride is 3840%.