A diver exhales a bubble with a volume of 255 mL at a pressure of 2.40 atm and a temperature of 7°C. What is the volume of the bubble when it reaches the surface where the pressure is 1.00 atm and the temperature is 25.0°C?

V₂ = 651.34 mL

Explanation:

Given data:

Initial volume = 255 mL

Initial pressure = 2.40 atm

Initial temperature = 7°C (7 +273 = 280 K)

Final temperature = 25°C (25 +273 = 298 k)

Final volume = ?

Final pressure = 1 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:

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 2.40 atm × 255 mL × 298 K / 280 K × 1 atm

V₂ = 182376 atm .mL. K / 280 K.atm

V₂ = 651.34 mL

it's all four options.