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A mixture of N2 and Ar gases in a cylinder contains 7 g of N2 and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of N2 is:
[Use atomic masses (in g mol–1): N=14,Ar=40]
[Use atomic masses (in g mol–1): N=14,Ar=40]
- a)12 bar
- b)15 bar
- c)18 bar
- d)9 bar
Correct answer is option 'B'. Can you explain this answer?
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Most Upvoted Answer
A mixture of N2 and Argases in a cylinder contains 7 gof N2and 8 gof A...
To find the partial pressure of N2, we need to calculate the mole fraction of N2 in the mixture.
First, we need to find the total number of moles of N2 and Ar in the mixture.
Moles of N2 = mass of N2 / molar mass of N2
Moles of N2 = 7 g / 28 g/mol = 0.25 mol
Moles of Ar = mass of Ar / molar mass of Ar
Moles of Ar = 8 g / 40 g/mol = 0.2 mol
Now, we can calculate the mole fraction of N2.
Mole fraction of N2 = moles of N2 / total moles
Mole fraction of N2 = 0.25 mol / (0.25 mol + 0.2 mol) = 0.5556
The partial pressure of N2 can be calculated using Dalton's law of partial pressures.
Partial pressure of N2 = mole fraction of N2 * total pressure
Partial pressure of N2 = 0.5556 * 27 bar = 14.9992 bar
Therefore, the partial pressure of N2 is approximately 15 bar.
First, we need to find the total number of moles of N2 and Ar in the mixture.
Moles of N2 = mass of N2 / molar mass of N2
Moles of N2 = 7 g / 28 g/mol = 0.25 mol
Moles of Ar = mass of Ar / molar mass of Ar
Moles of Ar = 8 g / 40 g/mol = 0.2 mol
Now, we can calculate the mole fraction of N2.
Mole fraction of N2 = moles of N2 / total moles
Mole fraction of N2 = 0.25 mol / (0.25 mol + 0.2 mol) = 0.5556
The partial pressure of N2 can be calculated using Dalton's law of partial pressures.
Partial pressure of N2 = mole fraction of N2 * total pressure
Partial pressure of N2 = 0.5556 * 27 bar = 14.9992 bar
Therefore, the partial pressure of N2 is approximately 15 bar.
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A mixture of N2 and Argases in a cylinder contains 7 gof N2and 8 gof Ar. If the total pressure of the mixture of the gases in the cylinder is 27bar, the partial pressure of N2is:[Use atomic masses (in g mol–1): N=14,Ar=40]a)12 barb)15 barc)18 bard)9 barCorrect answer is option 'B'. Can you explain this answer?
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