One step in the industrial production of nitric acid is oxidation of NO. 2NO(g)+

Question

One step in the industrial production of nitric acid is oxidation of NO. 2NO(g)+)O2(g) -> 2NO2(g) A reaction chamber is charged with 5.00 atm each of NO and O2. Calculate the final pressure of each participant if the reaction goes to completion without a change in temperature or volume.

Please provide full explanation not just answer.

One step in the industrial production of nitric acid is oxidation of NO. No, A reaction chamber is charged with 5.00 atm each of NO and O2. Calculate the final pressure of each participant if the reaction goes to completion without a change in temperature or volume. NO(g) NO2(g) O2(g) Number atm atm

Explanation / Answer

the reaction is 2NO+ O2-------->2NO2

Molar ratio of NO:O2= 2:1

since temperature and volume remains constant, n= PV/RT= 5V/RT for each NO and O2

So molar ratio of NO:O2= 5V/RT : 5V/RT= 1:1

limiting reactatant is NO ( since 2 mole are required and only one moles is supplied)

2 Moles of NO gives 2 moles of NO2 while consuming 1 mole of O2

5V/RT moles of NO gives 5V/RT moles of NO2 while consuming 2.5V/RT moles of O2

at the completation of reaction

moles of NO= 0 and hence pressure of NO=0 ( all the NO get consumed)

Moles of O2 remaining = 5V/RT-2.5V/RT= 2.5V/RT

moles of NO2 formed= 5V/RT

partial pressure of O2= nRT/V= 2.5VRT/VRT= 2.5 atm and partial pressure of NO2= 5 atm

partial pressure of NO= 0 ( since all the NO gets consumed).

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