In the first step of the Ostwald process for the synthesis of nitric acid, ammonia is converted to nitric oxide by the high-temperature reaction:4NH3(g)+5O2(g)+6H2O(g). How is the rate of consumption of O2 related to the rate of consumption of NH3?
To determine how the rate of consumption of O2 is related to the rate of consumption of NH3 in the given reaction, we need to examine the stoichiometry of the reaction.
The balanced equation for the reaction is: 4NH3(g) + 5O2(g) + 6H2O(g) → 4NO(g) + 6H2O(g)
From the balanced equation, we can see that the stoichiometric ratio between NH3 and O2 is 4:5. This means that for every 4 moles of NH3 consumed, 5 moles of O2 are consumed.
Based on this stoichiometric ratio, we can conclude that the rate of consumption of O2 is directly proportional to the rate of consumption of NH3. In other words, if the rate of consumption of NH3 increases by a certain factor, the rate of consumption of O2 will also increase by the same factor.
Therefore, the rate of consumption of O2 is directly related to the rate of consumption of NH3 in a proportion of 5:4.