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Subject ZIP Search Search Find an Online Tutor Now Ask Ask a Question For Free Login Chemistry Balancing Chemical Equations these 2 questions i need help with A chemist makes nitroglycerine, C3H5(NO3)3, from glycerol, C3H5(OH)3, and nitric acid according to the following balanced equation:C3H5(OH)3 + 3HNO3 → C3H5(NO3)3 + 3H2O a) In one experiment, 4.1 g of glycerol and 13.5 g of nitric acid produced 5.5 g of nitroglycerine. What was the percent yield of nitroglycerine? b) Offer a brief explanation as to why this reaction did not yield 100% products. Follow • 2 Add comment More Report

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Best Newest Oldest By: Best Newest Oldest C3H5(OH)3 + 3HNO3 → C3H5(NO3)3 + 3H2O Balanced equation a) moles glycerol used = 4.1 g x 1 mol/92.09 g = 0.0445 moles moles nitric acid used = 13.5 g x 1 mole/63.01 g = 0.214 moles Which is the limiting reagent? Mole ratio is 3 moles HNO3:1mole glycerol, thus glycerol is limiting. Based on the limiting reagent, 0.0445 moles glycerol --> 0.0445 moles nitroglycerine Theoretical mass of nitroglycerine = 0.0445 moles x 227 g/mole = 10.1 g nitroglycerine Actual yield = 5.5 g % yield = 5.5 g/10.1g (x100%) = 54.5% b) Possible explanation for less than 100% yield is that the product (nitroglycerine) is volatile, and so some will become vapor. Another possible reason is that perhaps the thermodynamics of the reaction (namely ∆G) is not favorable for the forward reaction even though the kinetics may be. Finally, if the reaction is reversible, there is little likelihood that 100% production will be achieved. Upvote • 0 Downvote Add comment More Report

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