Answer:
66.7%
Explanation:
The balanced equation for the reaction is given below:
2H2 + O2 —> 2H2O
Next, we shall determine the mass of O2 that reacted and the mass of H2O produced from the balanced equation. This is illustrated below:
Molar mass of O2 = 16x2 = 32g/mol
Mass of O2 from the balanced equation = 1 x 32 = 32g
Molar mass of H2O = (2x1) + 16 = 18g/mol
Mass of H2O from the balanced equation = 2 x 18 = 36g
Summary:
From the balanced equation above,
32g of O2 reacted to produce 36g of H2O.
Next, we shall determine the theoretical yield of H2O. This can be obtained as follow:
From the balanced equation above,
32g of O2 reacted to produce 36g of H2O.
Therefore, 100g of O2 will react to produce = (100 x 36)/32 = 112.5g of H2O.
Therefore, the theoretical yield of H2O is 112.5g
Finally, we shall determine the percentage yield of H2O as follow:
Actual yield = 75g
Theoretical yield = 112.5g
Percentage yield =?
Percentage yield = Actual yield /Theoretical yield x 100
Percentage yield = 75/112.5 x 100
Percentage yield = 66.7%
Therefore, the percentage yield of H2O is 66.7%
