the vapor pressure of pure water at 60 c is 157 mmHg. what is the vapor pressure of this solution at the same temperature, in mm Hg?
This appears not to be the complete question. It makes no sense as is.
To determine the vapor pressure of the solution at the same temperature, you need to know the concentration of solute in the solution. The vapor pressure of a solution is lower than the vapor pressure of the pure solvent due to the solute particles occupying some of the available surface area.
Once you know the concentration of the solute, you can use Raoult's Law to calculate the vapor pressure of the solution at the given temperature. Raoult's Law states that the vapor pressure of a solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent.
The equation for Raoult's Law is as follows:
Psolution = Xsolvent * Psolvent
Where:
Psolution is the vapor pressure of the solution.
Xsolvent is the mole fraction of the solvent.
Psolvent is the vapor pressure of the pure solvent.
Since you are given the vapor pressure of pure water at 60°C (157 mmHg), you need to find the mole fraction of water in the solution. Assuming the solute does not contribute significantly to the vapor pressure, the mole fraction of water can be calculated using the following formula:
Xsolvent = moles of water / total moles of solute and solvent
However, to find the vapor pressure of the solution accurately, you need additional information about the solute concentration or the number of moles of water and solute present in the solution.