Final answer:
The student needs to find the temperature of helium gas at a new pressure by applying the combined gas law. After converting units for pressure to atmospheres and temperature to Kelvin, the new temperature can be calculated and converted back to Celsius if needed.
Step-by-step explanation:
The student is asking for the temperature of a 42.0L canister of Helium gas at a pressure of 758 mmHg, given that the initial pressure is 112.0 kPa and the initial temperature is 25 degrees Celsius. To solve for the new temperature, we would use the combined gas law which relates the pressure, volume, and temperature of a fixed amount of gas:
P1/T1 = P2/T2
However, since the volume and the amount of gas do not change, the equation simplifies to:
P1/T1 = P2/T2
Before we can use this formula, we need to convert all of our units to be consistent. The initial pressure needs to be in atm (since 1 atm = 760 mmHg), and the temperatures need to be in Kelvin. The conversion for pressure from kPa to atm is given by:
P(atm) = P(kPa) / 101.325
After conversion and solving for the new temperature, you will get the final answer in Kelvin, which you can then convert back to Celsius if required.