a decompression chamber used by deep sea divers has a volume of 10.1m^3 and operates at an internal pressure of 4.25 atm. What volume, in cubic meters would the air in the chamber occupy if it were at 1.00 atm pressure, assuming no tempreature change.

V2=42.93cm3

Explanation:

According to Gay-Lussac's Law: "The Pressure Temperature Law. This law states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature. With an increase in temperature, the pressure will go up."

P1V1=P2V2

Given data

P1=4.25atm

V1=10.1cm³

P2=1atm

V2=?

V2=P1V1/P2

V2=(4.25*10.1)/1

V2=42.93cm3

see earlier answer