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Musya8 [376]
3 years ago
14

Two containers, one with a volume of 3.0 L and the other with a volume of 2.0 L contain, respectively, argon gas at 1.1 atm and

helium at 0.75 atm. The containers are initially separated by a valve, and then the valve is opened to connect the two containers. Assume perfect gases and determine the followings.
a. The total pressure of the mixed gases
b. The partial pressure of each gas
c. The mole fraction of each gas
Chemistry
1 answer:
aalyn [17]3 years ago
6 0

Answer:

a. p_T=0.93atm.

b.

p_{Ar}=0.66atm\\\\p_{He}=0.3atm

c.

x_{Ar}=0.6875\\\\x_{He}=0.3125

Explanation:

Hello,

In this case, considering that the valve is opened, we can use the Boyle's law in order to compute the final pressure of argon by considering its initial pressure and volume and a final volume of 5.0 L:

p_{Ar}=\frac{1.1atm*3.0L}{5.0L}=0.66atm

And the final pressure of helium:

p_{He}=\frac{0.75atm*2.0L}{5.0L}=0.3atm

Which actually are the partial pressure of both of them, it means that the total pressure is:

Finally, the mole fraction of each gas is computed by considering the Dalton's law:

x_i=\frac{p_i}{p_T}

x_{Ar}=\frac{0.66atm}{0.93atm} =0.6875\\\\x_{He}=\frac{0.3atm}{0.93atm} =0.3125

Best regards.

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