A balloon is filled with hydrogen at a temperature of 22.0 C and a pressure of 812 mm Hg. If the balloon's original volume was 1.25 liters, what will its new volume be at a higher altitude, where the pressure is only 625 mm Hg? Assume the temperature stays the same
Solution
The correct option is C
11.35 L
Pressure
P
1
= 1 bar, Volume
V
1
= 2.27 L
Pressure
P
2
= 0.2 bar, Volume
V
2
= To be calculated
As temperature remains constant at room temperature, applying Boyle’s Law,
P
1
V
1
=
P
2
V
2
(1 bar)(2.27 L) = (0.2 bar) (
V
2
)
V
2
=
2.27
0.2
= 11.35 L
Thus, the balloon can be expanded upto 11.35 L. Beyond this volume it will burst.