A gas mixture being used to simulate the atmosphere of another planet at 23°c consists of 337 mg of methane, 148 mg of argon, an

Question

1 year ago

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d 210 mg of nitrogen. The partial pressure of nitrogen at 296 k is 19. 0 kpa. Calculate the total pressure of the mixture.

1 answer:

Karolina [17] · Answer 1 · 2024-05-18T06:03:21+03:00

The total pressure of the mixture is 65.5 kPa.

According to Dalton's Law of Partial Pressure,

The partial pressure of gas = Mole fraction of gas × Total pressure

Total Pressure = Sum of all the gases partial pressures

The number of moles of methane is,

$Moles \: of \: methane \: (16 g/mol) = 337 \: mg \times \frac{1 g}{1000 mg} \times \frac{ 1 mol}{16 g }$

= 0.021 mols

The moles of methane are 0.021 mols.

The number of moles of the argon,

$Moles \: of \: argon (40 g/mol) = 148 \: mg \times \frac{ 1 g}{1000 mg } \times \frac{ 1 mol}{40 g}$

= 0.003 mols

The number of moles of argon is 0.003 mols.

The number of moles of nitrogen is,

$Moles \: of \: nitrogen (28 g/mol) = 296 \: mg \times \frac{ 1 g}{1000 mg} \times \frac{ 1 mol/}{28 g}$

= 0.010 mols

The number of moles of nitrogen is 0.010 mols.

The total number of moles is,

= 0.021 + 0.003 + 0.010

= 0.034 mols

$Mole \: fraction = \frac{ Moles \: of \: solute }{Total \: number \: of \: moles \: of \: soulte \: and \: solvent}$

$= \frac{ 0.010 }{ 0.034}$

= 0.29

$0.29 \: P _{total} = 19 \: kPa$

$P _{total} = \frac{ 19 \: kPa }{0.29}$

= 65.5 kPa

Therefore, the total pressure of the mixture is 65.5 kPa.

To know more about Dalton's law, refer to the below link:

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