Final answer:
Without additional context or details, we cannot determine the truthfulness of the statement about 193 mL of oxygen being collected. In a typical chemistry exercise, additional data such as temperature and water vapor pressure are necessary to calculate the dry gas pressure of the collected oxygen.
Step-by-step explanation:
The question provided describes a scenario where 193 mL of oxygen (O₂) gas is collected over water. To determine whether this statement could be true or false, we must consider the details provided in sample problems from chemistry exercises related to gas collection over water. However, the question alone does not contain enough information to determine its truthfulness since it lacks details like temperature and the vapor pressure of water at that temperature.
In related exercises, we often calculate the dry gas pressure by subtracting the water vapor pressure from the total atmospheric pressure. This would involve knowing the temperature and consulting a table for the vapor pressure of water at that temperature. The remaining pressure would be what the dry gas exerts. For example, if oxygen were collected at a total pressure of 762 mmHg, and the water vapor pressure at the collection temperature was given, these values could be used to find the dry pressure of the oxygen.