A 2.0L helium tank at a pressure of 15.0 kPa in a room kept at 22 degrees Celsius is used to blow up balloons....A 2.0L helium tank at a pressure...

There is a helium tank which can withstand a pressure of
15 kPa and has a volume of 2 L. It is kept at a temperature of 22 degree Celsius. The
balloons have a capacity of 2 L and can withstand 0.15 kPa without exploding. We need to
determine the maximum number of balloons that can be blown using the gas in the
tank.

We can apply the Ideal Gas Law to solve this problem.
The law gives the relation : P*V = n*R*T , where P is the pressure, V is the volume, n
is the amount of substance, R is the gas constant and T is the
temperature.

I assume the temperature of the gas does not
change when it is filled into the balloons.

The maximum
pressure that the balloon can withstand is 0.15 kPa and it has the same volume as that
of the tank. The reduction in pressure increases the volume of the gas. When the
pressure becomes 1/100, the volume becomes 100
times.

Therefore the gas can be used to fill 100 balloons.
The correct option is A.