Question

A 20 liter cylinder of helium at a pressure of 150 atm and a temperature of 27°C is used to fill a balloon at 1.00 atm and 37°C. What is the volume of the balloon?

A.
0.14 liters
B.
3000 liters
C.
2900 liters
D.
2400 liters
E.
3100 liters

Answer 1

Answer:The number of moles will remain the same in the two cases

so we can equate using ideal gas equation which is PV =nRT

V2 = 3100 L

Step-by-step explanation:

Answer 2

Answer: E. 3100 liters

Step-by-step explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

`(P_1V_1)/(T_1)=(P_2V_2)/(T_2)`

where,

`P_1` = initial pressure of gas = 150 atm

`P_2` = final pressure of gas = 1 atm

`V_1` = initial volume of gas = 20 L

`V_2` = final volume of gas = ?

`T_1` = initial temperature of gas =
`27^oC=273+27=300K`

`T_2` = final temperature of gas =
`37^oC=273+37=310K`

Now put all the given values in the above equation, we get the final pressure of gas.

`(150atm* 20L)/(300K)=(1atm* V_2)/(310K)`

`V_2=3100L`

Therefore, the volume of the baloon is 3100 L.