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The first step in the industrial production of nitric acid is reacting ammonia with oxygen according...

  1. The first step in the industrial production of nitric acid is reacting ammonia with oxygen according to the unbalanced equation:

    NH3(g) + O2(g) → NO(g) + H2O(g)
    How many liters of NH3(g) at 850.oC and 5.00 atm are required to react with 32.0 g of O2?

  2. 0.811g of KClO3 is decomposed as follows:
    2KClO3(s) → 2KCl(s) + 3O2(g)

    The O2 is collected over water at 28 oC and 765 torr. What is the volume of water displaced in this measurement, assuming the reaction goes to completion?

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