Final answer:
Without more information, it is not possible to determine the partial pressure of water vapor from the total pressure of 58 atm. Dalton's Law would require the partial pressures of other gases to solve this problem.
Step-by-step explanation:
To find the partial pressure of water vapor given a total pressure of 58 atm, we need additional information such as the partial pressures of other gases present or the specific temperature and humidity conditions if we are considering a water vapor equilibrium scenario. Unfortunately, without additional context or information, we cannot determine the partial pressure of water vapor just from the total pressure. Dalton's Law of Partial Pressures states that the total pressure of a mixture of gases is the sum of the partial pressures of the individual gases. To solve for the partial pressure of water vapor, we would need to know the partial pressures of the other gases in the mixture. However, if we are provided with the vapor pressure of water at a certain temperature, we could be dealing with a scenario where water vapor is the only gas present, or has reached its equilibrium vapor pressure at that temperature. In such a case, the partial pressure of water vapor would be equivalent to its vapor pressure at that temperature.