A gas sample is prepared in which the components have the following partial pressures: nitrogen, 555 mmHg; oxygen, 149 mmHg; water vapor, 13 mmHg; argon, 7 mmHg. What is the total pressure of this mixture?
Question
A gas sample is prepared in which the components have the following partial pressures: nitrogen, 555 mmHg; oxygen, 149 mmHg; water vapor, 13 mmHg; argon, 7 mmHg. What is the total pressure of this mixture?
Solution
The total pressure of a gas mixture can be found by adding up the partial pressures of all the individual gases. This is known as Dalton's Law of Partial Pressures.
Here are the steps to find the total pressure:
-
Identify the partial pressures of each gas:
- Nitrogen (N2): 555 mmHg
- Oxygen (O2): 149 mmHg
- Water vapor (H2O): 13 mmHg
- Argon (Ar): 7 mmHg
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Add up these partial pressures to find the total pressure:
- Total pressure = Pressure of N2 + Pressure of O2 + Pressure of H2O + Pressure of Ar
- Total pressure = 555 mmHg + 149 mmHg + 13 mmHg + 7 mmHg
- Total pressure = 724 mmHg
So, the total pressure of the gas mixture is 724 mmHg.
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