Chemistry · Chemical equations and stoichiometry
In the reaction when one mole of ammonia and one mole of oxygen are made to reac
In the reaction \( 4 N H_{3}+5 O_{2} \longrightarrow \) \( 4 N O+6 H_{2} O, \) when one mole of ammonia and one mole of oxygen are made to react to completion, then
- A. 1.0 mole of \( H_{2} O \) is produced
- B. All the oxygen is consumed
- C. 1.5 mole of \( N O \) is formed
- D. All the ammonia is consumed
Step-by-step solution
The balanced equation shows a 4:5 mole ratio of NH₃ to O₂. With 1 mole each, O₂ is limiting because it requires 1.25 moles of O₂ to fully react with 1 mole of NH₃, but only 1 mole is available. Thus, all oxygen is consumed, leaving some ammonia unreacted.
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