Ozone molecules in the stratosphere absorb much of the harmful radiation from the sun. typically, the temperature and partial pressure of ozone in the stratosphere are 250 k and 0.001 atm, respectively. how many grams of ozone are present in 1000 liters of air under these conditions? (assume ideal-gas behavior)

2.35 g of ozone are present

Explanation:

From Ideal gas equation,

PV = nRT equation 1

P = pressure of the ozone, n = number of mole of the ozone molecule, R = molar gas constant, V = volume of the ozone, T = Temperature.

making n the subject of the

n = PV/RT equation 2

Where V = 1000 dm³, P = 0.001 atm, T = 250 K, R = 0.082 atm/(dm³Kmol)

Substituting these values into equation 2

n = (1000×0.001)/(0.082×250)

n = 1/20.5

n = 0.049 mole.

Number of mole  = Reacting mass/ molar mass .

Molar mass of ozone gas (O₃) = 48 g/mol

Mass of Ozone = 48 × 0.049

Mass of ozone = 2.35 g.

Therefore, 2.35 g of ozone are present.

coral.

explanation:

coral. many marine organisms that produce calcium carbonate shells or skeletons are negatively impacted by increasing co2 levels and decreasing ph in seawater.

in the analysis of systems that involve fluid flow, we frequently encounter the combination of properties u and pv.