Geosmin is an aroma compound found in raindrops. It's chemical formula is C12H22O. The molar mass is 182 g/mol. If you perform combustion analysis of 1.77 grams of this compound, how many grams of carbon should be isolated as CO2 during the analysis?

5.13 g of CO₂.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

C₁₂H₂₂O + 17O₂ —> 12CO₂ + 11H₂O

Next, we shall determine the mass of C₁₂H₂₂O that reacted and the mass of CO₂ produced from the balanced equation. This can be obtained as follow:

Molar mass of C₁₂H₂₂O = 182 g/mol.

Mass of C₁₂H₂₂O from the balanced equation = 1 × 182 = 182 g

Molar mass of CO₂ = 12 + (2×16)

= 12 + 32

= 44 g/mol

Mass of CO₂ from the balanced equation = 12 × 44 = 528 g

SUMMARY:

From the balanced equation above,

182 g of C₁₂H₂₂O reacted to produce 528 g of CO₂.

Finally, we shall determine the mass of CO₂ produced from the reaction. This can be obtained as follow:

From the balanced equation above,

182 g of C₁₂H₂₂O reacted to produce 528 g of CO₂.

Therefore, 1.77 g of C₁₂H₂₂O will react to produce = (1.77 × 528)/182 = 5.13 g of CO₂.

Thus, 5.13 g of CO₂ were obtained from the reaction.

the answer is 0.8m.

by: nicholas

4d^55s^1 ( third choice)