Final answer:
The student is asked to calculate the number of moles of oxygen collected using the atmospheric pressure, vapor pressure of water, volume of the gas, and principles from the Ideal Gas Law.
Step-by-step explanation:
The student's question pertains to the collection of oxygen gas over water and involves applying the principles of gas collection and partial pressure to find the number of moles of oxygen collected. Given the total atmospheric pressure and the temperature at which the collection was done, we would first need to account for the vapor pressure of water at the given temperature to find the partial pressure of the dry oxygen gas. The vapor pressure of water at 23.0 °C is not provided, but it can be found from a standard reference table. Once the vapor pressure is known, it can be subtracted from the total atmospheric pressure to determine the partial pressure of the oxygen gas using Dalton's Law of Partial Pressures.
Then, apply the Ideal Gas Law, PV = nRT, where P is the pressure in atmospheres, V is the volume in liters, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/K·mol), and T is the temperature in Kelvin. By solving for 'n', we find the number of moles of O₂. The student's task is to carry out this calculation, requiring knowledge and application of gas laws and stoichiometry concepts from chemistry.