# Problem: 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 x 10–31 at 298 KUse 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%.

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###### FREE Expert Solution

We are asked to calculate the concentrations of nitrogen and oxygen present in air at a pressure of 1.0 atm and a temperature of 298 K assuming that nitrogen comprises 78% of air by volume and that oxygen comprises 21%.

To do so, we shall follow these steps:

Step 1: Determine the partial pressures and initial concentrations of the gases.

Step 2: Convert Kp to Kc.

Step 3: Construct an ICE chart and determine the equilibrium concentrations of the gases. ###### Problem Details
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 x 10–31 at 298 K
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%.