In the following reaction, how many grams of nitroglycerin c3h5(no3)3 will decompose to give 25 grams of co2? 4c3h5(no3)3(l) 12co2(g) 6n2(g) 10h2o(g) o2(g)

The balanced reaction that describes the decomposition of nitroglycerin to produce carbon dioxide, nitrogen, water and oxygen is expressed: 4c3h5(no3)3(l) = 12co2(g)+ 6n2(g) +10h2o(g) + o2(g). Hence for every 4 moles of nitroglycerin used, 12 moles of carbon dioxide is produced. When 25 grams of CO2 is produced, we convert this to mass and multiply by 4/12 and multiply again with the molar mass of nitroglycerin. The answer is 42.99 grams nitroglycerin.

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