Question

In alcohol fermentation, yeast converts glucose to ethanol and carbon dioxide.

C₆H₁₂O₆(s) 2C₂H₅OH(l) + 2CO₂(g)

If 5.97g of glucose reacts with 1.44 L of CO₂ gas is collected at 293 Kelvin and 0.984 atm what is the percent yield of the reaction ?

Answer 1

In alcohol fermentation, yeast converts glucose to ethanol and carbon dioxide. To calculate the percent yield, we compare the actual yield of carbon dioxide to the theoretical yield. The percent yield is calculated using the formula: (actual yield / theoretical yield) x 100%. Percent yield = 6.43%.

Step-by-step explanation:

In alcohol fermentation, yeast converts glucose (C6H12O6) to ethanol (C2H5OH) and carbon dioxide (CO2). The balanced chemical equation for this reaction is:

C6H12O6 → 2C2H5OH + 2CO2

To calculate the percent yield, we need to compare the actual yield to the theoretical yield. The actual yield is the amount of CO2 gas collected, which is given as 1.44 L. The theoretical yield can be calculated using stoichiometry. From the balanced equation, we can see that 1 mole of glucose produces 2 moles of ethanol and 2 moles of CO2. Therefore, the theoretical yield of CO2 can be calculated as:

Theoretical yield of CO2 = (moles of glucose) x (moles of CO2) = (mass of glucose / molar mass of glucose) x (moles of CO2 / moles of glucose) = (5.97 g / 180.16 g/mol) x (2 mol CO2 / 1 mol glucose) = 0.0663 mol CO2

Now, we can calculate the percent yield using the formula:

Percent yield = (actual yield / theoretical yield) x 100% = (1.44 L / 22.41 L/mol) x (0.0663 mol CO2 / 0.0663 mol CO2) x 100% = 6.43%