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The reaction of 9.50 g of carbon with Excess O2 Yield 12.8 of CO2. What is the percent yield of this reaction?
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Ngọc Khuê
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Answer:
Percentage yield = 36.75%
Explanation:
We’ll begin by writing the balanced equation for the reaction. This is illustrated below:
C + O₂ —> CO₂
Next, we shall determine the mass of C that reacted and the mass of CO₂ produced from the balanced equation. This can be obtained as follow:
Molar mass of C = 12 g/mol
Mass of C from the balanced equation = 1 × 12 = 13 g
Molar mass of CO₂ = 12 + (2×16)
= 12 + 32
= 44 g/mol
Mass of CO₂ from the balanced equation = 1 × 44 = 44 g
SUMMARY:
From the balanced equation above,
12 g of C reacted to produce 44 g of CO₂.
Next, we shall determine the theoretical yield of CO₂. This can be obtained as follow:
From the balanced equation above,
12 g of C reacted to produce 44 g of CO₂.
Therefore, 9.50 g of C will react to produce = (9.50 × 44) / 12 = 34.83 g of CO₂.
Thus, the theoretical yield of CO₂ is 34.83 g.
Finally, we shall determine the percentage yield of the reaction. This can be obtained as follow:
Actual yield of CO₂ = 12.8
Theoretical yield of CO₂ = 34.83 g
Percentage yield =?
Percentage yield = Actual yield / Theoretical yield × 100
Percentage yield = 12.8 / 34.83 × 100
Percentage yield = 1280 / 34.83
Percentage yield = 36.75%