8. The first step in the industrial manufacture of nitric acid is the oxidation of ammonia:4NH3(2 + 50ze) → 4 NO + 6 H20eIf 765.0g of O2 is used in excess ammonia, how many moles of each product are formed?

Given chemical reaction, 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O Mass of oxygen, O2 = 0.765 g…

The first step in the industrial manufacture of nitric acid is the oxidation of ammonia: 4NH32 + 502@ → 4 NO@ + 6 H2O@ If 765.0g of O2 is used in excess ammonia, how many moles of each product are formed?

The first step in the industrial manufacture of nitric acid is the oxidation of ammonia: 4NH32 + 502@ → 4 NO@ + 6 H2O@ If 765.0g of O2 is used in excess ammonia, how many moles of each product are formed?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.28PAE: 4.28 One of the steps in the manufacture of nitric acid is the oxidation of ammonia shown in this...

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Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

8. The first step in the industrial manufacture of nitric acid is the oxidation of ammonia:
4NH3(2 + 50ze) → 4 NO + 6 H20e
If 765.0g of O2 is used in excess ammonia, how many moles of each product are formed?

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