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3 Apr 2020
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 i parts (b) and (c) are consistent with the law of conservation of mass.
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 i parts (b) and (c) are consistent with the law of conservation of mass.
Sixta KovacekLv2
24 May 2020