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The pressure of a 1-L nitrogen gas sample at 25 ⁰C is 0.30 atm. The pressure of a 1-L oxygen gas sample at the same temperature is 0.25 atm. The oxygen gas sample is added to the nitrogen container. Argon gas is added to the mixture until the total pressure of the 1-L container reaches 1.00 atm, and the temperature is adjusted to 25 ⁰C. According to Dalton’s Law of Partial Pressures, the contribution of each gas to the total pressure of the gas mixture is: Nitrogen _____________ Oxygen _____________ Argon _____________

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onyebuchinnaji

Answer:

Nitrogen = 0.3 atm

Oxygen = 0.25 atm

Argon  = 0.45 atm

Explanation:

According to Dalton's law of partial pressure, the total pressure in the container is equal to sum of the partial pressures of the individual gases.

Given;

Total pressure of the gases, P_total = 1 atm

Pressure of nitrogen, P_nitrogen = 0.3 atm

Pressure of oxygen, P_oxygen = 0.25 atm

Pressure of argon, P_argon = ?

[tex]P_{total} = P_{nitrogen} + P_{oxygen} + P_{argon}\\\\1 \ atm= 0.3 \ atm + 0.25 \ atm + P_{argon}\\\\1 \ atm= 0.55 \ atm + P_{argon}\\\\ P_{argon} = 1 \ atm - 0.55 \ atm\\\\ P_{argon} = 0.45 \ atm[/tex]

Therefore, the contribution of each gas to the total pressure of the gas mixture is;

Nitrogen = 0.3 atm

Oxygen = 0.25 atm

Argon  = 0.45 atm

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