text: a bubble problem? a diver releases an air bubble of volume 2.0 cm^3 from a depth of 15 m below the surface of a lake, where the temperature is 7.0^oc. what is the volume of the bubble when it reaches just below the surface of the lake, where the temperature is 20^oc?  thanks, barbie okay, all annoying come-ons aside...  this is indeed an ideal gas law problem. here is how to solve it: pv=nrt p=pressure in atm v= volume in cm3 n= no of moles r= universal gas law constant t= temperature in kelvin  p1= 2atm p2 =1 atm v1= 2 cm3 v2= ????? t1= 7 c = 280k t2= 20 c= 293 k  so, it follows for p1v1=n1r1t1 that 2*2=nr *280 nr=4/280=0.0142857  then for p2v2=n2r2t2  1*v2=0.142857 *293 v2 = 4.19 cm3