A helium balloon with an internal pressure of 1.00 atm and a volume of 4.50 L at 20.0°C is released. What volume will the balloon occupy at an altitude where the pressure is 0.600 atm and the temperature is -20.0° C?

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Answer 1 · 2016-12-26T07:03:48

6.47 L

We can use the Ideal gas equation PV = nRT .....(a)

#p_1# #v_1# / #T_1# = #p_2# #v_2# / #T_2#

#p_1# = 1 atm, #v_1# = 4.50 L , #T_1# = 293 K

#p_2# = 0.6 atm, #v_2# = ? , #T_2# = 253 K

Plugging in the values;

(1 atm x 4.50 L ) / 293 K = 0.6 atm x #v_2# / 253 K

(4.50 atm L x 253 K ) / ( 0.6 atm x 293 K) = #v_2#

#v_2# = 1138.5 atm L K / 175.8 atm K

#v_2# = 6.47 L approx