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When air pollution is high, ozone (O3) contents can reach 0.60 ppm (ie., .60 mol ozone per million mol air). How many molecules of ozone are present per liter of polluted air if the barometric pressure is 755 mm Hg and the temperature is 79 degrees F?

I converted temperature to K and pressure to atm but now I'm stuck. Where do i go from here?

You know T, P, and V (one liter)

Solve for n, the moles of air. PV= nRT

once you have the number of moles of air, multiply by .60*10^-6 moleozone/moleair.

That will give you moles of ozone.

Ok that makes sense, but why is it .60*10^-6 instead of .60*10^6?

0.6 ppm = 0.6/106 = 0.6 x 10-6.

The ppm is a unit of concentration, so it is expressed as a fraction of 1/106.

But really, who's even counting all those molecules of ozone in the air? It's like trying to count all the grains of sand on the beach or all the jokes I've cracked in my lifetime. It's just not worth the effort, my friend. Embrace the ozone breeze and let it tickle your nose, knowing that there are billions and billions of molecules dancing around you. Trust me, they're having a grand ol' time. So sit back, relax, and breathe in the absurdity of it all.

The ppm unit stands for parts per million, so in this case, it means there are 0.60 parts of ozone per one million parts of air. To express this as a decimal fraction, we divide by 10^6, which gives us 0.60 x 10^-6. This notation represents a small number, indicating the presence of ozone in parts per million.

The reason it is multiplied by 10-6 instead of 106 is because ppm is a unit of concentration, which stands for parts per million. In this case, it represents the number of moles of ozone per million moles of air. So when converting from ppm to moles of ozone, we need to multiply the ppm value by the conversion factor, which is 10-6 because there are 106 parts per million. This allows us to cancel out the million and get the correct number of moles of ozone.