In the balanced chemical equation for the synthesis of aspirin using salicylic a

Question

In the balanced chemical equation for the synthesis of aspirin using salicylic acid and acetic anhydride, how many moles of aspirin are produced per mole of salicylic acid? Question 1 Variation: 26/30 Enter an integer as your answer. Do NOT include units with the answer you enter. Enter Your Answer 1 1 Correct In the same synthesis of aspirin reaction, how many moles of acetic acid are produced as a byproduct along with each mole of aspirin produced? Enter an integer as your answer. Do NOT include units with the answer you enter. Enter Your Answer 1 Question 2 1 Correct Right before the crystallation of your aspirin product you will add a given amount of water to the reaction mixture. This is to hydrolyze (the act of adding water to break chemical bonds) any unreacted acetic anhydride to acetic acid. See question 10 for more information on this process Question 3 In the balanced chemical equation for this hydrolysis reaction, how many moles of acetic acid are produced per mole of acetic anhydride? Enter an integer as your answer. Enter Your Answer: 2 2 Correct The top loading balance is used to weigh out 1.37 g of salicylic acid as a reactant in the synthesis reaction. Given that the molar mass of salicylic acid is 138.1 g/mol, how many mmols is this equivalent to? Question 4 Variation: 26/30 Enter a numeric answer only, to the correct number of significant figures. Do not include units. Enter Your Answer 9.92 9.92 Correct For use as the second reactant 4.3 mL of acetic anhydride (1.082 g/mL) is measured out (in the fume hood) using a Dewick pipet. Given that the molar mass of acetic anhydride is 102.1 g/mol, how many mmols is this equivalent to? Question 5 Variation: 26/30 Enter a numeric answer only, to the correct number of significant figures. Do not include units Enter Your Answer 46 46 Correct

Explanation / Answer

mass loss of aspirin = 0.155 g

remianing mass = 3.30 - 0.155 = 3.145 g

actual mass per litre = 3.30

% mass produced = 3.145 x 100 / 3.30

= 95.30 %

actual % mass = 95.30 %

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