1. The problem statement, all variables and given/known data At an altitude of 50 km, the average atmospheric temperature is 0C. what is the average number of air molecules per cm^3 of air at this atmosphere? Given formula: P(sub h) = P(sub 0) x e^(-Mgh/RT) = -(Mgh x 10^5)/2.303RT Assuming P = 1 atm at sea level and h in km M=28.97g/mol=28.97cm^3/mol g = 9.81 m/s^2 = .0981 km/s^2 h = 50 km R = 8.314 J/K•mol = 82.06cm^3•atm/K•mol T = 0 C = 273.15 K I'm having trouble because using the scale height form of the equation (second form) I get lost in the units, and I'm receiving an error on my TI using the first. 3. The attempt at a solution Using second equation: Log P(sub h) = (-Mgh x 10^5)/2.303RT = -(28.97)(.0981)(50)(10^5)/ (2.303)(82.057)(273.15) = -275.28 10^(-275.28) = 5.23... But the units after the conversion don't add up ... Suggestions?