5. 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 of H2O form? (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed? (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

5. 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 of H2O form? (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed? (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Example: Consider the following balanced reaction: 4 Al (s) + 3 O2 (g) → 2 Al2O3 (s) If 5.60 mol of Al (26.98 g/mol) and 3.10 mol of O₂ (32.00 g/mol) react to form 178 g Al2O3 (101.96 g/mol); (a) What is the maximum number of grams of Al2O3 that can be produced? (b) What is the limiting reactant? (c) How many grams of excess reactant are left over? (d) What is the percent yield?
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