Nitrogen oxide is a pollutant in the lower atmosphere that irritates the eyes an

Question

Nitrogen oxide is a pollutant in the lower atmosphere that irritates the eyes and lungs and leads to the formation of acid rain. Nitrogen oxide forms naturally in atmosphere according to the endothermic reaction

N2(g)+O2(g)2NO(g)

Kp=4.1×1031 at 298 K.

Part A

Use the ideal gas law to calculate the concentrations of nitrogen and oxygen present in air at a pressure of 1.0 atm and a temperature of 298 K. Assume that nitrogen comprises 78% of air by volume and that oxygen comprises 21%.

Part B

Find the "natural" equilibrium concentration of NO in air in units of molecules/cm3.

Explanation / Answer

we can assume that 1L sample

  N2(g) + O2(g) <--> 2NO(g)
I= 0.78M 0.21M 0M

C= -X -X +2X

E= 0.78-X 0.21-X 2X
  

to setup the equation I would use this. ([NO]-2)/[N2][O2]= 4.1*10^-31

so ([2X]^2)/(0.78-X)(0.21-X)=4.1*10^-31

A accurate possibly positive only calculation gives me 1.295*10^-16  
4X^2 = (6.7158*10^-32) - (4.059*10^-31)X + (4.1*10^-31)X^2

(4.1*10^-31)X^2 number .  .

+/- 1.2957*10^-16.

the value of X

so 0.78-1.2957*10^-16= 0.78M of N2
and 0.21 -1.2957*10^-16= 0.21M of O2

ideal gas law used here

P= 1.0 ATM
v= assumed 1L
N=?
R=(0.08206)
T=298K

Solving for N gets me 0.04089 mol of gases

N2 and o2 =QUESTION mark

P=1.0atm
V= .78L of N2
N=?
R=(0.08206)
T=298K
solving for N gets me 0.03189 mols of N2

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