if oxygen gas were collected over water at 22c and the total pressure of the wet gas were 710 mm hg what would be the partial pressure of the oxygen?
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To calculate the partial pressure of oxygen gas collected over water at 22°C, you need to consider the vapor pressure of water at that temperature. The partial pressure of oxygen is determined by subtracting the vapor pressure of water from the total pressure.
First, find the vapor pressure of water at 22°C, which is obtained from the water vapor pressure table. At 22°C, the vapor pressure of water is approximately 19.8 mmHg.
Next, subtract the vapor pressure of water from the total pressure of the mixture to obtain the partial pressure of oxygen:
Partial pressure of oxygen = Total pressure – Vapor pressure of water
Partial pressure of oxygen = 710 mmHg – 19.8 mmHg
Partial pressure of oxygen = 690.2 mmHg
Therefore, the partial pressure of oxygen gas in the wet gas collected over water at 22°C is approximately 690.2 mmHg.
To determine the partial pressure of oxygen in a gas collected over water, you need to account for the pressure exerted by water vapor using Dalton's Law of Partial Pressure. Here's how you can find the partial pressure of oxygen:
1. Look up the vapor pressure of water at the given temperature. At 22°C, the vapor pressure of water is approximately 19.8 mmHg.
2. Subtract the vapor pressure of water from the total pressure of the wet gas. In this case, subtract 19.8 mmHg from 710 mmHg:
Partial pressure of oxygen = Total pressure of wet gas - Vapor pressure of water
Partial pressure of oxygen = 710 mmHg - 19.8 mmHg
Partial pressure of oxygen ≈ 690.2 mmHg
Therefore, the partial pressure of oxygen in the gas collected over water at 22°C would be approximately 690.2 mmHg.