Question

A balanced reaction for conversion of ammonia to nitric oxide by catalytic oxidation of ammonia is:

• A. ${4NH}_3+{5O}_2\underset{Pt}{\overset{{800}^{0}C}{\to }}4NO+6H_{2}O+△$
• B. ${4NH}_3+{3O}_2\underset{Pt}{\overset{{800}^{0}C}{\to }}4NO+2H_{2}O+△$
• C. ${2NH}_3+{5O}_2\underset{Pt}{\overset{{800}^{0}C}{\to }}2NO+6H_{2}O+△$
• D. ${4NH}_3+{4O}_2\underset{Pt}{\overset{{800}^{0}C}{\to }}4NO+4H_{2}O+△$

Answer 1

The correct option is A ${4NH}_3+{5O}_2\underset{Pt}{\overset{{800}^{0}C}{\to }}4NO+6H_{2}O+△$

${4NH}_3+{5O}_2\underset{Pt}{\overset{{800}^{0}C}{\to }}4NO+6H_{2}O+△$
The catalyst used is platinum. The catalyst glows since the catalytic oxidation of ammonia is an exothermic reaction. The industrial process is known as Ostwald's Process for the manufacture of nitric acid.