The oxygen gas emitted from an aquatic plant during photosynthesis is collected over water at a temperature of 25 degrees celsius and a total pressure of 762 torr. What is the partial pressure of the oxygen gas?
What formula do I need to use?
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To find the partial pressure of the oxygen gas, you can use Dalton's law of partial pressures, which states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases.
The formula for Dalton's law of partial pressures is:
P(total) = P1 + P2 + P3 + ...
In this case, the total pressure is given as 762 torr. The partial pressure of the oxygen gas is what we need to find.
Since the oxygen gas is collected over water, we need to take into account the vapor pressure of water at 25 degrees Celsius. At this temperature, the vapor pressure of water is approximately 24 torr.
Therefore, the partial pressure of the oxygen gas can be calculated as follows:
Partial pressure of oxygen gas = Total pressure - Vapor pressure of water
Partial pressure of oxygen gas = 762 torr - 24 torr
Partial pressure of oxygen gas = 738 torr
So, the partial pressure of the oxygen gas is 738 torr.