Industrial production of nitric acid, which is used in many products including fertilizers and explosives, approaches 10 billion kg per year worldwide. The first step in its production is the exothermic oxidation of ammonia, represented by the following equation. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) ΔH⁰rxn = −902.0 kJ If this reaction is carried out using 7.007 ✕ 103 g NH3 as the limiting reactant, what is the change in enthalpy?
Industrial production of nitric acid, which is used in many products including fertilizers and explosives, approaches 10 billion kg per year worldwide. The first step in its production is the exothermic oxidation of ammonia, represented by the following equation. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) ΔH⁰rxn = −902.0 kJ If this reaction is carried out using 7.007 ✕ 103 g NH3 as the limiting reactant, what is the change in enthalpy?
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 61PS: The standard enthalpy of formation of solid barium oxide, BaO, is 553.5 kJ/mol, and the standard...
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Industrial production of nitric acid, which is used in many products including fertilizers and explosives, approaches 10 billion kg per year worldwide. The first step in its production is the exothermic oxidation of ammonia, represented by the following equation.
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
ΔH⁰rxn
= −902.0 kJIf this reaction is carried out using 7.007 ✕ 103 g NH3 as the limiting reactant, what is the change in enthalpy?
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