The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia: NH3 (g) + O2 (g) ---> No (g) + NO (G) + H2O (g) The equation is unbalanced. The reaction is run using 824 g NH3 and excess oxygen. How many moles of NO are formed? How many moles of H2O are formed?

Which is not true regarding reaction rates? (2 points) catalysts are not used up in the reaction. catalysts speed up reactions by lowering the activation energy. reaction rates decrease as the concentration of reactants decrease. during reactions, concentrations of all reactants decrease at the same rate.