In one experiment 6.50 grams or salicylic acid is reacted with excess acetic any

Question

In one experiment 6.50 grams or salicylic acid is reacted with excess acetic anyone. The reaction produces 7.10 grams of acetylsalicylic acid, calculate the percent yield for the experiment. How many grams of salicylic acid must be used in order to produce 5.00 grams of acetylsalicylic acid (aspirin) assuming that the reaction yield is only 92.0%? (Assuming excess acetic anhydride) What is the minimum number of milliliters of acetic anhydride required to react with 3.50 grams of salicylic acid? The density of acetic anhydride is given on the data sheet.

Explanation / Answer

1) moleculer weight of salicylic acid is 138.12 g/mol

moleculer weight of acetyl salicylic acid is 180.157 g/mol

Percent yield =obtained yield/theoretical yield × 100

actual theoretical yield =weight of product(acetyl salicylic acid)/weight of starting material(salicylic acid)*weight of starting material taken

actual theoretical yield=180.157/138.12*6.5

actual theoretical yield=8.478 g

so percentage yield =weight obtained/theoretical yield*100

percentage yield =7.1/8.478*100

percentage yield=83.74

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