$n=$ number of moles

$R=$ ideal gas constant

$T=$ temperature

A different form of this equation is often used in atmospheric science

$p=N{k}_{b}T$

where

$p=$ pressure $($mbar$)$

$N=$ number density $($or concentration$)($molecules $\frac{?}{c{m}^3})$

$K_b=$ Boltzmann's constant $(1\mathrm{.}38{10}^{-19}\frac{m}{b}ar*K^{-1}*c{m}^3)$

$T=$ temperature $($Kelvin$)$

From this form of the ideal gas law, you can determine the number of air molecules in $1$ cubic centimeter of

air. If you are given temperature in Celsius or Fahrenheit, you'll need to convert those numbers into a less

well known temperature scale called Kelvin.

To convert from Celsius to Kelvin

$T(K)=273\mathrm{.}15+T(C)$

For example, a temperature of $20C$ would be $293\mathrm{.}15K.$

To convert from Fahrenheit to Kelvin is a bit more complicated

$T(K)=\frac{5}{9}**(T(F)-32)+273\mathrm{.}15$

For example, a temperature of $70F$ is equal to $294\mathrm{.}261K$

Using this information, determine the density of the atmosphere at three different places in the atmShow your work and use scientific notation $(2,000,000=2{10}^6)$

a$)$ The surface

b$)$ The top of the surface inversion layer

c$)$ The tropopause