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17 Nov 2019
one step in the commercial process for the converting ammonia to nitric acid is the conversion of NH3 to NO:
NH3(g) + O2(g) -------------} NO(g) + H2O(g)
In certain experiment 2.00 g of NH3 reacts with 2.50 g of O2. (a)Is the reaction equation balanced? (If not, balanced it).(b) What is the limiting reactant? (c)How many grams of NO and H2O form?
one step in the commercial process for the converting ammonia to nitric acid is the conversion of NH3 to NO:
NH3(g) + O2(g) -------------} NO(g) + H2O(g)
In certain experiment 2.00 g of NH3 reacts with 2.50 g of O2. (a)Is the reaction equation balanced? (If not, balanced it).(b) What is the limiting reactant? (c)How many grams of NO and H2O form?
Hubert KochLv2
14 Feb 2019