The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: N₂(g) + O₂(g) 2 NO(g) If 13.32 g N₂ is mixed with 16.35 g O₂, calculate the theoretical yield (g) of NO produced by the reaction. Submit Submit Answer Show Approach Show Tutor Steps Try Another Version 10 item attempts remaining Approach masses of reactants Step 1 amount (mol) reactants Step 2 limiting reactant, and amount (mol) product Step 3 Step 1 Calculate the amount (mol) of each reactant initially present using the molar mass of each reactant. Step 4 Calculate the mass of product formed based on the molar mass of the product. amount (mol) product Step 4 mass of product Ⓡ Step 2 Compare the ratio of amounts of reactants present to the ratio of the stoichiometric coefficients of the reactants to determine which is the limiting reactant. Step 3 Calculate the amount (mol) of product formed by complete consumption of the limiting reactant.

The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: N₂(g) + O₂(g) 2 NO(g) If 13.32 g N₂ is mixed with 16.35 g O₂, calculate the theoretical yield (g) of NO produced by the reaction. Submit Submit Answer Show Approach Show Tutor Steps Try Another Version 10 item attempts remaining Approach masses of reactants Step 1 amount (mol) reactants Step 2 limiting reactant, and amount (mol) product Step 3 Step 1 Calculate the amount (mol) of each reactant initially present using the molar mass of each reactant. Step 4 Calculate the mass of product formed based on the molar mass of the product. amount (mol) product Step 4 mass of product Ⓡ Step 2 Compare the ratio of amounts of reactants present to the ratio of the stoichiometric coefficients of the reactants to determine which is the limiting reactant. Step 3 Calculate the amount (mol) of product formed by complete consumption of the limiting reactant.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 121QRT: Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A...

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Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
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