A meteorological balloon contains 250.0 l he at 22°c and 740.0mmhg if the volume of the balloon can vary according to external conditions what volume would it occupy at an altitude at which the temperature is - 52°c and the pressure is 0.750 atm

243.15 l

Explanation:

Using the general gas law

P₁V₁/T₁ = P₂V₂/T₂

V₂ = P₁V₁T₂/P₂T₁ where P₁, V₁ and T₁ are the initial pressure, volume and temperature of the meteorological balloon and P₂, V₂ and T₂ are the initial pressure, volume and temperature of the meteorological balloon.

P₁ = 740 mmHg V₁ = 250 l and T₁ = 22°C + 273 = 295 K,

P₂ = 0.750 atm = 0.750 * 760 mmHg = 570 mmHg (since 1 atm = 760 mmHg) and T₂ = - 52°C + 273 = 221 K

V₂ = P₁V₁T₂/P₂T₁ = 740 mmHg * 250 l * 221 K/570 mmHg * 295 K = 243.15 l

V₂ = 243.15 l

So the volume it would occupy at an altitude of temperature - 52 °C where it pressure is 0.750 atm is 243.15 l