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A 2.00 kg sample of ammonia is mixed with 4.00 kg of oxygen. Which is the limiting reagent and how much excess reactant remains on completion of the reaction? What is the theoretical yield of NO. The equation below represents this reaction. If only 1.65 kg of NO are produced what is the percent yield of NO?
____ NH3(g) + ____ O2(g) â ____ NO(g) + ____ H2O(g)
A 2.00 g sample of ammonia reacts with 4.00 g of oxygen according to the equation
4NH3+5O2→4NO+6H2O.
How much excess reactant remains after the reaction has stopped?
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.