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OpenStudy (elleblythe):
Solid ammonium nitrate decomposes explosively to form nitrogen gas, oxygen gas, and water vapor. Assume 100% yield. a. Write a stoichiometric relationship between the reactant and products. Answer: 2NH4NO3-->2N2+1O2+4H2O ? b. How many moles are there in 3.00 g of ammonium nitrate? A: 0.037mol NH4NO3 ? c. How many moles of each of the three products are produced when 3.00 g of ammonium nitrate decomposes? d. How many grams of each product are produced? A: 0.14g N2, 0.031g O2, 0.89g O2 ? e. What is the total mass of the three products? Is the Law of Conservation of Mass obeyed?
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