Final answer:
To find the volume of neon gas at standard temperature with constant pressure, Charles’s Law is applied. However, considering the conditions match standard temperature and pressure (STP), it’s known any gas at STP has a molar volume of 22.4 L/mol. Thus, the volume the neon gas would occupy at STP is 22.4 L.
Step-by-step explanation:
The student's question pertains to the behavior of a gas under different temperature conditions while keeping the pressure constant. To determine what volume neon gas would occupy at standard temperature, we must apply Charles’s Law, which states that the volume of a gas is directly proportional to its temperature when pressure is held constant. Given that the volume of the gas at 25°C (or 298K) is 752 ml, we need to find out what the volume would be at 0°C (or 273K), the standard temperature.
Firstly, we need to convert the temperatures from Celsius to Kelvin by adding 273.15 to the Celsius temperature. Then, we can use Charles’s Law in the form V1/T1 = V2/T2 to solve for V2, where V1 is the initial volume (752 ml), T1 is the initial temperature (298K), and T2 is the standard temperature (273K). Solving for V2 gives us the volume of the gas at standard temperature. However, we know that we do not need to perform these calculations in this specific case because any gas at STP (Standard Temperature and Pressure), which includes a temperature of 273K and a pressure of 1 atm, has a molar volume of 22.4 L/mol. Therefore, the answer to the student's question is a) 22.4 L, given the conditions are at STP, which align with our problem's assumption of constant pressure and a change to standard temperature.