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Answer:
11.73 Kg of CO₂
Explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
2C₈H₁₈ + 25O₂ —> 16CO₂ + 18H₂O
Next, we shall determine the mass of C₈H₁₈ that reacted and the mass of CO₂ produced from the balanced equation. This can be obtained as follow:
Molar mass of C₈H₁₈ = (12×8) + (18×1)
= 96 + 18
= 114 g/mol
Mass of C₈H₁₈ from the balanced equation = 2 × 114 = 228 g
Convert 228 g to kg.
1000 g = 1 Kg
Therefore,
228 g = 228 g × 1 Kg / 1000 g
228 g = 0.228 Kg
Molar mass of CO₂ = 12 + (16×2)
= 12 + 32
= 44 g/mol
Mass of CO₂ from the balanced equation = 16 × 44 = 704 g
Convert 704 g to Kg
1000 g = 1 Kg
Therefore,
704 g = 704 g × 1 Kg / 1000 g
704 g = 0.704 Kg
SUMMARY:
From the balanced equation above,
0.228 Kg of C₈H₁₈ reacted to produce 0.704 Kg of CO₂.
Finally, we shall determine the mass of carbon dioxide, CO₂, that will be produced by the reaction of 3.8 kg of octane, C₈H₁₈. This can be obtained as follow:
From the balanced equation above,
0.228 Kg of C₈H₁₈ reacted to produce 0.704 Kg of CO₂.
Therefore, 3.8 kg of C₈H₁₈ will react to produce = (3.8 × 0.704) / 0.228 = 11.73 Kg of CO₂
Thus, 11.73 Kg of CO₂ is added to the atmosphere per 3.8 kg of C₈H₁₈.