Ammonia reacts with O2 to form either NO(g) or NO2(g) according to these unbalanced equations: NH3(g) O2(g) ⟶NO(g) H2O(g) NH3(g) O2(g) ⟶NO2(g) H2O(g) In a certain experiment, 2.00 moles of NH3(g) and 10.00 moles of O2(g) are contained in a closed flask. After the reaction is complete, 6.75 moles of O2(g) remains. Calculate the number of moles of NO(g) in the product mixture. (Hint: You cannot do this problem by adding the balanced equations, because you cannot assume that the two reactio
Ammonia reacts with O2 to form either NO(g) or NO2(g) according t…
May 12, 2020
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Take the reaction: NH3 O2 NO H2O. In an experiment, 3.25 g of NH3 are allowed to react with 3.50 g of O2. (i) Which reactant is the limiting reagent? (ii) How many grams of NO are formed? (iii) How much of the excess reactant remains after the reaction?
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Balance the following important equation: NH3 O2 → NO H2O (catalytic oxidation of NH3) - Chemistry | Shaalaa.com
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4 NH3 (g) 5 O2 (g) → 4 NO (g) 6 H2O (l)a) If you react 9.25 g of ammonia (NH3) with excess oxygen, how many grams of water are produced?b) If you react 44.28 L of oxygen with excess ammonia (NH3), how many liters of NO are produced?c) If you produce 28.14 g of water, how many molecules of ammonia did you consume?d) If 12.39 L of oxygen is consumed, what is the theoretical yield in grams of water?
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