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Aspirin can be prepard from salicylic acid (C_(7)H_(6)O_(3)) and acetic anhydride (C_(4)H_(6)O_(3)) according to the equation 2C_(7)H_(6)O_(3)+C_(4)H_(6)O_(3)rarr2C_(9)H_(8)O_(4)+H_(2)O This reaction gives a yield of 74%, provided that a 50% excess of acetic anhydride (the cheaper reagent) is used. If a chemist wants to prepare 20.0g of aspirin in the laboratory, what mass of the of acetic anhydride should be use ? |
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Answer» `20.7g` If 100% YIELD 360g of Asprine required`=102g` of acetic anhydried 1G of Asprine required `=(102)/(360)g` of acetic anhydried 20g of Asprine required `=(102)/(360)xx20g` of acetic anhydried But for 74% yield acetic anhydride required is =7.657g But CHEMIST taking 50% exceeds, So `=7.65+7.65xx(500)/(100)=11.5g` |
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