Calculating Volume of Air for Nitrogen Dioxide Dillution

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To calculate the volume of air needed to dilute HNO3 to 0.050 ppm from 560 g of NO2, the reaction equation indicates that 4 moles of NO2 produce 4 moles of HNO3. Using the ideal gas law (V=nRT/P), the volume of HNO3 gas produced is first determined. A dilution ratio is then applied, leading to a calculated air volume of approximately 5.9 x 10^9 liters. This calculation assumes constant temperature and pressure conditions. The solution appears to be correct based on the calculations provided.
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Homework Statement


Nitrogen dioxide reacts with water in the atmosphere to produce acid rain.
4N02(g)+2H20(g)+O2(g)------> 4HNO3(g)
assuming that the temperature and the pressure remain constant, calculate the volume of air at 1 atm, 20oC, necessary to dilute the HNO3(g) to 0.050 ppm(by volume) when 560.g of NO2(g) is allowed to react.

Homework Equations



V=nRT/P where n=number of moles, R=ideal gas constant, T=temperature, P= pressure

The Attempt at a Solution



First calculate the volume of HNO3 gas that will be produced. then using the equation a/b=c/d
I calculated the volume required to dilute

.050L/1,000,000L = 292.808L / V

solve for V and I got 5.9 x 10^9 L
 
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Looks OK.
 
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