Oxidation of Benzaldehyde 3. A short discussion of yields. Imagine that you had
ID: 1026717 • Letter: O
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Oxidation of Benzaldehyde 3. A short discussion of yields. Imagine that you had a small apple orchard and thb coe produce a maximum of 2400 apples per season. This number of apples is the t ideal yield of your orchard orchard can a. In the first year, everything goes pretty well and the or chard produced, or yielded 2345 apples. This is the actual yield of your orchard yield by the theoretical yield. If you multiply this percent efficiency or percent yield of your orchard Percent Yield = 2345 apples x 100 = 97.7 % b. Quantitatively, you can calculate the efficiency of your orchard by dividing the number by 100 you wil get the c. In the second year, you harvested 2110 apples out of the same orchard. What was the percent yield of your orchard in the second year? 0400 4. In chemistry, the percent yield of reactions can be calculated from the molar stoichiometry of reactions. For example, the conversion of glucose to fructose occurs in a 1:1 molar ratio as shown below Glucose- Fructose MW 180 g/mole 180 g/mole ed to fructose and 0.80 moles of fructose is collected, a. at is the percent yield of the reaction? If 0.50 moles of glucose are converted to fructose and 0.20 moles of fructose is collected, what is the percent yield of the reaction? b· 5. In today's experiment, benzaldehyde is oxidized by potassium permanganate to potassium benzoate, a salt of benzoic acid. a. Draw the structure of potassium benzoate below 62Explanation / Answer
Ans 3c
In second year
% yield = actual yield x 100 / theoretical yield
= 2110*100/2400
= 87.916%
Ans 4 a
From the stoichiometry of the reaction
1 mol of glucose can produce = 1 mol of fructose
Theoretical yield of fructose = 1 mol
Actual yield of fructose = 0.80 mol
% yield = actual yield x 100 / theoretical yield
= 0.80*100/1
= 80%
Ans 4b
From the stoichiometry of the reaction
1 mol of glucose can produce = 1 mol of fructose
0.50 mol of glucose can produce = 0.50 mol of fructose
Theoretical yield of fructose = 0.50 mol
Actual yield of fructose = 0.20 mol
% yield = actual yield x 100 / theoretical yield
= 0.20*100/0.50
= 40%
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