Question

Dalton’s Law CalculationA mixture of H₂, N₂ and Ar gases is present in a steel cylinder. The total pressure within the cylinder is 675 mm Hg and the partial pressures of N₂ and Ar are, respectively, 354 mm Hg and 235 mm Hg. If CO₂ gas is added to the mixture, at constant temperature, until the total pressure reaches 842 mm Hg, what is the partial pressure, in mm Hg, of the following?A) CO₂, 167 B) N₂, 354 C) Ar, 235 D) H₂, 8629

Answer 1

Answer:

A) The partial presssure of CO₂ is 167 mm Hg

B) The partial presssure of N₂ is 354 mm Hg

C) The partial presssure of Ar is 235 mm Hg

D) The partial presssure of H₂ is 86 mm Hg

Explanation:

Dalton's law of partial pressures is basically expressed by the following statement:

The total pressure of a mixture is equal to the sum of the partial pressures of its components.

So initially we have:

$P_{T}$= total presure of the system (675 mm Hg).

$P_{N_2}$= partial pressure of N₂ (354 mm Hg).

$P_{Ar}$= partial pressure of Ar (235 mm Hg).

Using Dalton's law we can find the partial pressure of H₂:

$P_{T}=P_{N_2}+P_{Ar}+P_{H_2}$

675 mm Hg=354 mm Hg + 235 mm Hg + $P_{H_2}$

$P_{H_2}$= 675 mm Hg - 354 mm Hg - 235 mm Hg

$P_{H_2}$=86 mm Hg

If CO₂ gas is added to the mixture, at constant temperature, and the volume is the same, the difference between the new total pressure and the previous total pressure is equal to the partial pressure of CO₂.

$P_{T}=P_{N_2}+P_{Ar}+P_{H_2}+P_{CO_2}$

842 mm Hg= 354 mm Hg + 235 mm Hg + 86 mm Hg + $P_{CO_2}$

$P_{CO_2}$= 842 mm Hg - 354 mm Hg - 235 mm Hg - 86 mm Hg

$P_{CO_2}$= 167 mm Hg