A sample of nitrogen gas is collected over water at 20°C. The vapor pressure of water at 20°C is 18 mmHg. What is the partial pressure of the nitrogen if the total pressure is 765 mmHg?

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A sample of nitrogen gas is collected over water at 20°C. The vapor pressure of water at 20°C is 18 mmHg. What is the partial pressure of the nitrogen if the total pressure is 765 mmHg?

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Answer 1 · 2016-06-13T05:09:07

$P_"measured"=P_"SVP"+P_"Gas"$

Explanation:

$P_"SVP"$ is the saturated vapour pressure, which is the vapour pressure of water, and is extensively tabulated across a range of temperatures. Of course, at $100$ $""^@C$ the saturated vapour pressure is $1$ $atm$ . Why?

So if we want $P_"Gas"$ (which we do), all we have to do is subtract $P_"SVP"$ from $P_"measured"$

$P_"measured"-P_"SVP"$ $=$ $P_"Gas"$ $=$ $(765-18)*mm*Hg$

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A sample of nitrogen gas is collected over water at 20°C. The vapor pressure of water at 20°C is 18 mmHg. What is the partial pressure of the nitrogen if the total pressure is 765 mmHg?

1 Answer

Explanation:

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