Question

The electrolysis of water forms H2 and O2.
2H2O → 2H2 + O2
What is the percent yield of Oz if 10.2 g of Oz is produced from the decomposition of 17.0 g of H20?
Actual yield
Use %Yield = =
Theoretical yield To
15.1%
33.8%
60.1%
67.6%

Answer 1

Answer:

67.5% ≅ 67.6%

Explanation:

Given data:

Mass of water = 17.0 g

Mass of oxygen produced  (actual yield)= 10.2 g

Percent yield of oxygen = ?

Solution:

Chemical equation:

2H₂O   →   2H₂ + O₂

Number of moles of water:

Number of moles = mass/ molar mass

Number of moles = 17.0 g/ 18.016 g/mol

Number of moles = 0.944 mol

Now we will compare the moles of oxygen with water to know the theoretical yield of oxygen.

                        H₂O       :        O₂

                          2          :         1

                        0.944      :      1/2×0.944 = 0.472 mol

Mass of oxygen:

Mass = number of moles× molar mass

Mass = 0.472 mol × 32 g/mol

Mass = 15.104 g

Percent yield:

Percent yield = [Actual yield / theoretical yield] × 100

Percent yield = [ 10.2 g/ 15.104 g] × 100

Percent yield = 0.675 × 100

Percent yield = 67.5%

Answer 2

Answer:

67.6

Explanation: