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Two baloons are at the same temperature and pressure. one contains 8g of helium and the other contain 80g of argon

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If there is a question you are not asking it.
Now let us try to find out what the question might have been.
Assuming that both gases follow the ideal gas law, we have for both gases PV=nRT where P is the pressure, V the volume, T the absolute temperature, R the gas constant, and n the number of moles.
Let subscript _1 refer to the Helium gas and _2 to the Argon gas. You can write

  1. P_1*V_1=n_1*R*T_1
  2. P_2*V_2=n_2*R*T_2
Divide the left sides one by the other and do the same for the right sides. Since P_1=P_2 and T_1=T_2 there are cancellations and you are left with
(V_1/V_2)=(n_1/n_2)
That is all you can say: The ratio of the volumes is equal to the ratio of the numbers of moles.
Now using the molar masses of the gases (M_1=4 g, and M_2=40 g) you find n_1 is about 2 moles and n_2 is also about 2 moles. The conclusion is that the two balloons have approximately the same volume.
Note:You can use more accurate molar masses for the gases but that will not change the conclusion.
The question should have been: What is the ratio of the volumes of the balloons?

Posted on Apr 26, 2013

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