Final answer:
To find the temperature at which the volume of the oxygen sample will be 1.00 L at 0.500 atm, the combined gas law is used, yielding a final temperature of 500.25 K after converting Celsius to Kelvin and ensuring volume units match.
Step-by-step explanation:
The student's question involves finding the temperature at which a given sample of oxygen will have a volume of 1.00 L and a pressure of 0.500 atm, given its initial conditions of 300.0 mL, 1.00 atm, and 27.0°C. To solve this problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas: P1V1/T1 = P2V2/T2, where P1 and P2 are the initial and final pressures, V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures in Kelvin.
To find the final temperature T2, we rearrange the formula: T2 = (P2V2T1)/(P1V1). First, convert the initial temperature from Celsius to Kelvin by adding 273.15, so T1 is 300.15 K. Then plug in the values: T2 = (0.500 atm * 1.00 L * 300.15 K) / (1.00 atm * 0.300 L) = 500.25 K. Therefore, the sample of oxygen will be at a temperature of 500.25 K.
Note: It is crucial to convert all temperatures to Kelvin and volumes to the same units before solving.