Nitrogen dioxide reacts with water and oxygen in the atmosphere to produce acid rain.
4NO2(g) + 2H2O(g) + O2(g) = 4HNO3(g)
Assuming that the temperature and the pressure remain constant, calculate the volume of air at 1 atm, 20 C, necessary to dilute the HNO3(g) to 0.080 ppm (by volume) when 532 g of NO2(g) is allowed to react.
I am wondering what should I do with the 0.080 ppm. I am pretty sure I know how to do everything else but, I am not sure how to use the ppm in to the equation of if it used after the pv=nRT equation.
I would calculate mols HNO3 produced by 532 g NO2 and substitute into PV = nRT and solve for L HNO3 at the temperature and pressure.
Then ppm = L HNO3/1,000,000 L air at 20C.
0.08E-6 = LHNO3 produced/x
Solve for x = L air
Check my thinking.
To calculate the volume of air necessary to dilute HNO3(g) to 0.080 ppm (parts per million), you will need to use the ideal gas law equation, PV = nRT.
Let's break down the steps to solve the problem:
1. Convert the amount of NO2(g) to moles: To do this, you need the molar mass of NO2, which is 46.0055 g/mol. Divide the given mass (532 g) by the molar mass to find the number of moles of NO2:
moles of NO2 = 532 g / 46.0055 g/mol
2. Determine the number of moles of HNO3 produced: From the balanced chemical equation, you can see that 4 moles of NO2 produce 4 moles of HNO3. Therefore, the number of moles of HNO3 will be the same as the moles of NO2.
3. Calculate the volume of HNO3(g) based on its concentration: The given concentration is 0.080 ppm, which means there are 0.080 parts of HNO3 for every 1 million parts of air. To convert this to a ratio of moles of HNO3 to moles of air, divide 0.080 ppm by 1 million:
moles of HNO3 / moles of air = 0.080 ppm / 1,000,000
4. Calculate the volume of air: Since the pressure (P) and temperature (T) are constant, you can rewrite the ideal gas law equation as V = (nRT) / P. Rearrange the equation to solve for V:
V = (moles of air * R * T) / P
Plug in the values of moles of air (from step 3), the gas constant (R = 0.0821 L·atm/(K·mol)), the given temperature (20°C = 293.15 K), and 1 atm for pressure.
Note: Make sure to use consistent units throughout the calculation.
By following these steps, you can obtain the volume of air necessary to dilute the HNO3(g) to 0.080 ppm.