Aballoon filled with helium gas at 20 °c occupies 4.91 l at 1.00 atm. the balloon is immersed in liquid nitrogen at -196°c, raising the pressure to 5.20 atm. what is the volume of the balloon in the liquid nitrogen?
a) 0.25 l
b) 3.6 l
c) 6.7 l
d) 97 l

(A)0.25L

Explanation:

By combination of Boyle's law and Charles law to obtain the general gas equation, we have:

P1V1/T1=P2V2/T2

P1=Inital pressure=1.00 atm

V1=Inital volume=4.91L

T1=Initial temperature=20°C=20+273=293Kelvin

P2=Final pressure=5.2atm

T2=Final temperature=(-196+273K)=77K

V2= final volume=?

by making V2 the subject of the above general gas equation

we have V2=P1V1T2/P2T1

=1×4.91×77/5.2×293

=0.248L

the answer is the first option

explanation:

just googled it m8. not that hard

lol

i believe it is a.) released into

explanation: