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Chemistry, 12.07.2019 02:30, Thejollyhellhound20
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, 1.90 g of nh3 reacts with 2.30 g of o2. (a) which is the limiting reactant? o2 nh3 (b) how many grams of no and of h2o form? 1.73 g no 1.55 g h2o (c) how many grams of the excess reactant remain after the limiting reactant is completely consumed? g (d) show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass. mass of products + excess reactant g total mass of reactants g
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One of the steps in the commercial process for converting ammonia to nitric acid is the conversion o...
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