Enter Your Answer In The Provided Box Using The Balanced Equ

Enter Your Answer In The Provided Box1using The Balanced Equatio

Using the balanced equation for fermentation: C₆H₁₂O₆ (aq) → 2 C₂H₆O (aq) + 2 CO₂ (g)

Calculate the grams of ethanol formed from 0.50 mol of glucose:

From the balanced equation, 1 mol of glucose produces 2 mol of ethanol. The molar mass of ethanol (C₂H₆O) is approximately 46.07 g/mol.

Total ethanol produced = 0.50 mol × 2 mol ethanol / mol glucose = 1 mol ethanol.

Mass of ethanol = 1 mol × 46.07 g/mol = 46.07 grams.

Answer: 46.07 g C₂H₆O

Paper For Above instruction

The fermentation process of glucose to ethanol and carbon dioxide is a fundamental biochemical reaction. The balanced chemical equation C₆H₁₂O₆ (aq) → 2 C₂H₆O (aq) + 2 CO₂ (g) illustrates the stoichiometry involved. Using this equation, we can perform quantitative calculations to determine the amount of products formed from given quantities of reactants.

Firstly, when calculating ethanol production from glucose, the mole ratio is key. Since 1 mol of glucose yields 2 mol of ethanol, the amount of ethanol generated can be directly calculated from the moles of glucose provided. For 0.50 mol of glucose, the number of moles of ethanol produced is 1 mol. Multiplying this by ethanol's molar mass (approximately 46.07 g/mol), we find that around 46.07 grams of ethanol are formed. This demonstrates how stoichiometry, molar mass, and balanced equations work together to facilitate precise quantitative analyses in biochemical processes.

Secondly, to determine the amount of carbon dioxide produced from 0.15 mol of glucose, the same molar ratio applies. From the balanced equation, 1 mol of glucose produces 2 mol of CO₂. Therefore, 0.15 mol of glucose yields 0.30 mol of CO₂. The molar mass of CO₂ is approximately 44.01 g/mol, so the mass of CO₂ produced is 0.30 mol × 44.01 g/mol = 13.20 grams. This calculation emphasizes the importance of understanding mole ratios and molar masses for accurate product quantification in fermentation reactions.

Thirdly, when determining the amount of glucose needed to produce a specific amount of ethanol, the reverse calculation applies. Since 2 mol of ethanol are produced per mol of glucose, producing 5.2 mol of ethanol requires 2.6 mol of glucose. Given that the molar mass of glucose (C₆H₁₂O₆) is approximately 180.16 g/mol, the mass of glucose needed is 2.6 mol × 180.16 g/mol ≈ 468.42 grams. This showcases how stoichiometric conversions can determine reactant requirements for desired product yields.

In the context of organic synthesis, the reaction between salicylic acid and acetic anhydride to produce aspirin is well characterized: C₇H₆O₃ (salicylic acid) + C₂H₄O₃ (acetic anhydride) → C₉H₈O₄ (aspirin) + H₂O. Accurate mass calculations involve similar stoichiometric principles. To find the grams of aspirin formed from 37.9 grams of salicylic acid, we first determine the molar amount of salicylic acid (about 138.12 g/mol). The molar ratio from the balanced equation is 1:1, so the molar amount of aspirin formed is equivalent to the molar amount of salicylic acid used, approximately 0.2745 mol. Multiplying by the molar mass of aspirin (180.16 g/mol), yields about 49.46 grams of aspirin.

Similarly, calculating the amount of acetic acid needed involves the same molar ratio, producing the same molar quantity as salicylic acid. The molar mass of acetic acid (C₂H₄O₂) is approximately 60.05 g/mol. For 73.6 g of salicylic acid (which is about 0.533 mol), the same mol of acetic acid (0.533 mol) is needed, corresponding to roughly 32.0 grams of acetic acid.

Lastly, the amount of water formed in this reaction can be calculated based on the molar ratios. From the balanced equation, 1 mol of salicylic acid reacts to produce 1 mol of water. For 59.1 g of salicylic acid (about 0.427 mol), an equivalent mol of water is formed, which weighs approximately 19.23 grams (since the molar mass of water is 18.015 g/mol).

These calculations demonstrate how stoichiometry and balanced chemical equations are essential tools in chemical quantification, applicable broadly across biochemical and organic synthesis processes.

References

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