120 ml of oxygen gas was collected over water at a barometric pressure of 732.0 torr and 23 degrees celsius. what is the partial pressure of the oxygen?
Ptotal = PO2 + PH2O
Ptotal = 732.0 torr.
pH2O = vapor pressure H2O (look in tables in your text) @ 23 degrees C.
Solve for PO2.
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To find the partial pressure of oxygen, we need to consider the vapor pressure of water at the given temperature and subtract it from the total barometric pressure. Here's how to calculate it step by step:
Step 1: Look up the vapor pressure of water at 23 degrees Celsius. Note that the vapor pressure changes with temperature. At 23 degrees Celsius, the vapor pressure of water is approximately 21.1 torr.
Step 2: Subtract the vapor pressure of water from the total barometric pressure to get the partial pressure of oxygen. In this case, the total barometric pressure is given as 732.0 torr. So, the partial pressure of oxygen can be calculated as:
Partial pressure of oxygen = Total barometric pressure - Vapor pressure of water
Partial pressure of oxygen = 732.0 torr - 21.1 torr
Partial pressure of oxygen = 710.9 torr
Therefore, the partial pressure of oxygen in this case is 710.9 torr.