Question

Be sure to answer all parts. Ozone molecules in the stratosphere absorb much of the harmful radiation from the sun. How many ozone molecules are present in 5.00 L of air under the stratospheric ozone conditions of 251 K temperature and 1.79 × 10−3 atm pressure

Answer 1

there are 0.00043484598 mol of ozone molecules

Step-by-step explanation:

To find how many molecules of ozone there are in those conditions we have to apply the ideal gas law P×V = n×R×T

Where P stands for Pressure of the gas, V for volume, n is for the amount of gas in moles, R for the universal gas constant which is 0.082 atm×l\ K×mol and T stands for temperature in Kelvin.

if we replace what with the information:

P×V=n×R×T

1.79×10-3 ×5l = n × 0.082 atm×l ×251K

K×mol

0,00895 atm×l = n × 20.582 atm×l

mol

we pass 20.582 atm×l to the other side

mol

0.00895 atm×l = n

20.582 atm×l\mol

we divide and simplify atm ×l with atm× l and the result is:

0.00043484598 mol=n

Answer 2

There are
`2.6172 * 10^(20)` molecules of ozone present in 5.00 L of air under the stratospheric ozone conditions of 251 K temperature and
`1.79 * 10^(-3)` atm pressure.

Step-by-step explanation:

To find the number of molecules of ozone you need to:

1. Use the Ideal Gas equation to find the moles of ozone and,
2. Use the Avogadro number (
   `6.02214* 10^(23)`) to find the molecules of ozone.

Given

`V= 5.00 \:L\\T=251 \:K\\P=1.79 * 10^(-3) \:atm`

The Ideal Gas equation is

`PV=nRT`

solving for n

`n=(PV)/(RT)`

where

`R=0.08205 \:(L\cdot atm)/(mol \cdot K)`

Substituting the values given into the expression we derived for n, we obtain

`n=((1.79 * 10^(-3) \:atm)\cdot (5.00 \:L))/((0.08205 \:(L\cdot atm)/(mol \cdot K))\cdot (251 \:K))= 4.346* 10^(-4) \:mol`

Find the number of molecules of ozone

`4.346* 10^(-4) \:mol \cdot 6.02214* 10^(23)\:(molecules)/(mol) =2.6172 * 10^(20) \:molecules`