One of the steps in the industrial production of nitric acid is the combustion of NO at room temp...
one of the steps in the industrial production of nitric acid is the combustion of NO at room temperature:
2NO +O2 <--> 2NO2. Kp= 4.2X10^12.
A reactor is filled with 10.0 atm of each of NO and O2.
a) calculate the equilibrium pressure of NO2.
b) calculate the equilibrium constant pressure of NO
**please show how to find the answer
Homework Answers
Value of Kp is large, reaction is almost complete. According to stoichiometry of reaction, moles of NO2 formed equal to moles of NO(g) reacted.
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One of the steps in the industrial production of nitric acid is the combustion of NO at room temp...
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The oxidation of nitric oxide NO + 02 =NO2 takes place in an isothermal batch reactor. The reactor is charged with a mixture containing 20.0 volume percent NO and the balance air at an initial pressure of 380 kPa (absolute). (a) Assuming ideal-gas behavior, determine the composition of the mixture (component mole fractions) and the final pressure (kPa) if the conversion of NO is 90%. (b) Suppose the pressure in the reactor eventually equilibrates (levels out) at 360 kPa. What...
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