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Zielflug [23.3K]
3 years ago
8

A weather balloon is filled with helium that occupies a volume of 500 L at 0.995 atm and 32.0 ℃. After it is released, it rises

to a location where the pressure is 0.720 atm and the temperature is -12 ℃. What is the volume of the balloon at the new location?
Chemistry
1 answer:
Yuki888 [10]3 years ago
3 0

Answer : The volume of the balloon at the new location is, 591.3 L

Explanation :

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

The combined gas equation is,

\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}

where,

P_1 = initial pressure of gas = 0.995 atm

P_2 = final pressure of gas = 0.720 atm

V_1 = initial volume of gas = 500 L

V_2 = final volume of gas = ?

T_1 = initial temperature of gas = 32.0^oC=273+32=305K

T_2 = final temperature of gas = -12^oC=273+(-12)=261K

Now put all the given values in the above equation, we get:

\frac{0.995atm\times 500L}{305K}=\frac{0.720atm\times V_2}{261K}

V_2=591.3L

Therefore, the volume of the balloon at the new location is, 591.3 L

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