One of the steps in the commercial process for convertingammonia to nitric acid is the conversion of NH3 to NO:4 NH3(g) + 5 O2(g)------>4 NO(g) + 6 H2O(g)In a certain experiment, 2.00 g of NH3 reacts with 2.50 g ofO2. (a) Which is the limiting reactant? (b) How many gramsof NO and H2O form? (c) How many grams of the excess reactantremain after the limiting reactant is completely consumed?(d) Show that your calculations in parts (b) and (c)are consistent with the law of conservation of mass.

During chemical reactions, compound that possess lesser moles in comparison to others (according to…

Answered: One of the steps in the commercial…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 70QRT

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One of the steps in the commercial process for converting
ammonia to nitric acid is the conversion of NH₃ to NO:
4 NH3(g) + 5 O₂₍g)------>4 NO(g) + 6 H₂O(g)
In a certain experiment, 2.00 g of NH₃ reacts with 2.50 g of
O₂. (a) Which is the limiting reactant? (b) How many grams
of NO and H₂O form? (c) How many grams of the excess reactant
remain after the limiting reactant is completely consumed?
(d) Show that your calculations in parts (b) and (c)
are consistent with the law of conservation of mass.

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