Aballoon filled with 750.0 ml of helium at a temperature of 25 degrees celsius and an atmosphere pressure of 745 mm hg. what volume will the balloon have when it reaches an altitude where the temperature is -35 degrees celsius and the pressure is 0.60 atm?

V₂ = 0.98 L

Explanation:

Given data:

Initial volume = 750 mL  =0.75 L

Initial pressure = 745 mmHg (745/760 =0.98 atm)

Initial temperature = 25 °C (25 +273 = 298 K)

Final temperature = -35°C (-35+273 = 238 K)

Final volume = ?

Final pressure = 0.60 atm

Formula:

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

P₁V₁/T₁ = P₂V₂/T₂  

V₂ = P₁V₁T₂/T₁ P₂

V₂ = 0.98 atm × 0.75 L × 238 K / 298 K × 0.60 atm

V₂ = 174.93 atm .L. K / 178.8  K.atm

V₂ = 0.98 L

the formula would be mgso4

mgso[subscript]4

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