The partial pressure of N 2 in the air is 593 mmHg at 1 atm. What is the partial pressure of N 2 in a bubble of air a scuba diver breathes when he is 66 ft below the surface of the water where the pressure is 3.00 atm?

The partial pressure of nitrogen in the air is 593 millimeters of mercury at 1 atmosphere. What is the partial pressure of nitrogen in a bubble of air a scuba diver breathes when he is 66 feet below the surface of the water where the pressure is 3 atmospheres? Alright. So realize here that we can work with proportions to solve this. Realize that the pressure of 593 millimeters of mercury is connected to the 1 atmosphere. So we're gonna say 593 millimeters of mercury per 1 atmosphere. We're gonna say that equals, we don't know what the new pressure is, but we know that we don't know what the new, partial pressure of nitrogen is, but we know that pressure is now 3 atmospheres. So all we got to do now is solve for the missing x. So cross multiply these 2, cross multiply these 2. So when we do that we're gonna get 1 atmosphere times x equals 593 millimeters of mercury times 3 atmospheres, divide both sides here by 1 atmosphere. Atmospheres cancel out and I'll be left with millimeter millimeters of mercury for nitrogen gas. So here, it would equal 1779 millimeters of mercury. So here, this would be the answer for the partial pressure of my nitrogen gas at a new pressure of 3 atmospheres.

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8. Gases, Liquids and Solids

Dalton's Law: Partial Pressure (Simplified)

GOB Chemistry

8. Gases, Liquids and Solids

Dalton's Law: Partial Pressure (Simplified)

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Multiple Choice

The partial pressure of N₂ in the air is 593 mmHg at 1 atm. What is the partial pressure of N₂ in a bubble of air a scuba diver breathes when he is 66 ft below the surface of the water where the pressure is 3.00 atm?

2.34 mmHg

1779 mmHg

593 mmHg

2.28×10³ mmHg

7.02 mmHg

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Verified step by step guidance

Understand that the partial pressure of a gas in a mixture is proportional to the total pressure of the mixture. This is described by Dalton's Law of Partial Pressures.

Identify the initial conditions: the partial pressure of N2 at the surface is 593 mmHg when the total pressure is 1 atm (760 mmHg).

Recognize that the total pressure at 66 ft below the surface is 3.00 atm. Convert this pressure to mmHg: 3.00 atm × 760 mmHg/atm = 2280 mmHg.

Use the ratio of pressures to find the new partial pressure of N2: (Partial Pressure of N2 at depth) = (Partial Pressure of N2 at surface) × (Total Pressure at depth / Total Pressure at surface).

Calculate the partial pressure of N2 in the bubble at 66 ft depth using the formula: (593 mmHg) × (2280 mmHg / 760 mmHg).