Answer:
53.4%
Step-by-step explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
N2 + 3H2 —> 2NH3
Next, we shall determine the mass of H2 that reacted and the mass of NH3 produced from the balanced equation. This is illustrated below:
Molar mass of H2 = 2 × 1.01 = 2.02 g/mol
Mass of H2 from the balanced equation = 3 × 2.02 = 6.06 g
Molar mass of NH3 = 14 + (3×1.01)
= 14 + 3.03
= 17.03 g/mol
Mass of NH3 from the balanced equation = 2 × 17.03 = 34.06 g
Summary:
From the balanced equation above,
6.06 g of H2 reacted to produce 34.06 g of NH3.
Next, the shall determine the theoretical yield of NH3. This can be obtained as follow:
From the balanced equation above,
6.06 g of H2 reacted to produce 34.06 g of NH3.
Therefore, 26.3 g of H2 will react to produce = (26.3 × 34.06)/6.06 = 147.82 g of NH3.
Thus, the theoretical yield of NH3 is 147.82 g
Finally, we shall determine the percentage yield of NH3. This is illustrated below:
Actual yield = 79 g
Theoretical yield = 147.82 g
Percentage yield =.?
Percentage yield = Actual yield /Theoretical yield × 100
Percentage yield = 79/147.82 × 100
Percentage yield of NH3 = 53.4%