Final answer:
The volume of a sample of oxygen gas at a pressure of 2.00 atm and 27°C is calculated to be 6.723 L when the pressure is changed to 453 mm Hg (0.595 atm) at the same temperature using Boyle's Law.
Step-by-step explanation:
The student's question relates to the calculation of a gas's volume at a different pressure while maintaining the same temperature using the ideal gas law. According to the question, a sample of oxygen gas occupies a volume of 2.00 L at a pressure of 2.00 atm and a temperature of 27°C (300 K approx). The student wants to know the volume of the gas at a pressure of 453 mm Hg (which is equivalent to 0.595 atm) at the same temperature.
To solve this, we can use Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume at constant temperature (P1V1 = P2V2). Here's how to calculate the new volume:
V2 = (P1 x V1) / P2
V2 = (2.00 atm x 2.00 L) / 0.595 atm
V2 = 4.00 L / 0.595 atm
V2 = 6.723 L (rounded to three decimal places)
Therefore, the sample of oxygen gas will occupy a volume of 6.723 L at a pressure of 453 mm Hg at the same temperature.