In the fermentation process, yeast converts glucose to ethanol and carbon dioxide. What volume of carbon dioxide, measured at 745 torr and 25.0°C,

Question

In the fermentation process, yeast converts glucose to ethanol and carbon dioxide. What volume of carbon dioxide, measured at 745 torr and 25.0°C, can be produced by the fermentation of 10.0 g of glucose? C6H12O6(aq) → 2C2H5OH(aq) + 2CO2(g)

Answer 1

I just answered this for someone else, but I would caution that I am not certain this is correct:

First, we have to convert torr to atm, °C to °K, and grams of glucose to moles of carbon dioxide.

745 torr x (0.00131579 atm / 1 torr) = 0.98 atm

25°C + 273.15 = 298.15°K

10g C₆H₁₂O₆ x (1 mol / 180.156g) = 0.06 mol C₆H₁₂O₆ x (2 mol CO₂ / 1 mol C₆H₁₂O₆) = 0.12 mol CO₂

Second, we can use the ideal gas law equation to find the unknown pressure.

P V = n R T

(0.98) (V) = (0.12) (0.08206) (298.15)

0.98V = 2.94

V = 2.94 / 0.98

V = 3L

Answer:

3 liters of carbon dioxide, measured at 745 torr and 25.0°C, can be produced by the fermentation of 10.0 g of glucose.