Respuesta :
Explanation:
The given data is as follows.
Number of particles of diatomic gas = 3
Number of particles of monoatomic gas = 6
Number of particles of another monoatomic gas = 5
Therefore, total number of particles or moles present will be as follows.
3 + 6 + 5 = 14
As we know that, mole fraction = [tex]\frac{\text{moles of given substance}}{\text{total no. of moles}}[/tex]
Hence, more fraction of the diatomic gas will be as follows.
mole fraction = [tex]\frac{\text{moles of given substance}}{\text{total no. of moles}}[/tex]
= [tex]\frac{3}{14}[/tex]
= 0.21
Now, formula to calculate partial pressure will be as follows.
Partial pressure of one species = molar fraction of that species x total pressure
Therefore, [tex]P_{diatomic} = \text{mole fraction diatomic} \times P_{total}[/tex]
[tex]P_{total} = \frac{0.330 atm}{0.21}[/tex]
= 1.57 atm
Thus, we can conclude that total pressure is 1.57 atm.
The total pressure of the gaseous mixture is 1.57 atm.
The mixture of the gases consists of 3 diatomic molecules, 6 monoatomic molecules, and 5 other monoatomic molecules.
The total number of molecules in the mixture are:
[tex]\rm Total\;molecules\;=\;3+6+5\\Total\;molecules\;=\;14[/tex]
Computation for the total pressure of the gas
The total pressure of a gas by Raoult's law is given as:
[tex]\rm Total\;pressure=\dfrac{Partial\;pressure}{Mole\;fraction}[/tex]
The partial pressure of the diatomic gas is 0.330 atm.
The mole fraction of the diatomic gas is given as:
[tex]\rm Mole\;fraction=\dfrac{Molecules\;of\;diatomic\;gas}{Total\;molecules} \\\\Mole\;fraction=\dfrac{3}{14}\\\\ Mole\;fraction=0.2[/tex]
The mole fraction of the diatomic gas is 0.2.
The total pressure of the gas is given as:
[tex]\rm Total\;pressure=\dfrac{0.330}{0.2}\;atm\\\\ Total\;pressure=1.57\;atm[/tex]
The total pressure of the gaseous mixture is 1.57 atm.
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