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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

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boffeemadrid

Answer:

0.25 L

Explanation:

[tex]P_1[/tex] = Initial pressure = 1 atm

[tex]T_1[/tex] = Initial Temperature = 20 °C

[tex]V_1[/tex] = Initial volume = 4.91 L

[tex]P_2[/tex] = Final pressure = 5.2 atm

[tex]T_2[/tex] = Final Temperature = -196 °C

[tex]V_2[/tex]= Final volume

From ideal gas law we have

[tex]\dfrac{P_1V_1}{T_1}=\dfrac{P_2V_2}{T_2}\\\Rightarrow V_2=\dfrac{P_1V_1T_2}{T_1P_2}\\\Rightarrow P_2=\dfrac{1\times 4.91(273.15-196)}{(20+273.15)\times 5.2}\\\Rightarrow V_2=0.24849\ L\approx 0.25\ L[/tex]

The pressure experienced by the balloon is 0.25 L

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