Question

A balloon 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, while the pressure is raised to 5.20 atm. What is the volume of the balloon in the liquid nitrogen?a. 97 Lb. 6.7 Lc. 3.6 Ld. 0.25 L

Answer 1

0.25 L

Step-by-step explanation:

`P_1` = Initial pressure = 1 atm

`T_1` = Initial Temperature = 20 °C

`V_1` = Initial volume = 4.91 L

`P_2` = Final pressure = 5.2 atm

`T_2` = Final Temperature = -196 °C

`V_2`= Final volume

From ideal gas law we have

`(P_1V_1)/(T_1)=(P_2V_2)/(T_2)\\\Rightarrow V_2=(P_1V_1T_2)/(T_1P_2)\\\Rightarrow P_2=(1* 4.91(273.15-196))/((20+273.15)* 5.2)\\\Rightarrow V_2=0.24849\ L\approx 0.25\ L`

The pressure experienced by the balloon is 0.25 L