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 7.056 ✕ 103 g nh3 as the limiting reactant, what is the change in enthalpy?

Achemical equilibrium between gaseous reactants and products is shown. n2(g) + 3h2(g) ⇌ 2nh3(g) how will the reaction be affected if the pressure on the system is increased? it will shift toward the reactant side as there is lower pressure on the reactant side. it will shift toward the product side as there is higher pressure on the product side. it will shift toward the reactant side as there are a greater number of moles of gas on the reactant side. it will shift toward the product side as there are a fewer number of moles of gas on the product side.