Final answer:
In accordance with Gay-Lussac's law, if the pressure of a gas increases from 545 torr to 724 torr, while maintaining a constant volume, the temperature in Celsius increases from 118°C to approximately 247.5°C.
Step-by-step explanation:
This particular question is based on Gay-Lussac's law which states that for a given amount of gas at a constant volume, the pressure of the gas is directly proportional to its absolute temperature. The formula for this law is P1/T1 = P2/T2, where P stands for pressure and T represents absolute temperature in Kelvin.
So, to find the new temperature, first we need to convert the initial temperature from Celsius to Kelvin (T1 = 118+273 = 391 K). Then we substitute the pressure and temperature values into the equation: 545/391 = 724/T2.
Solve for T2 and we get T2 = 724*391/545 ≈ 520.5 K. We need to convert this to degrees Celsius by subtracting 273, so T2 will be approximately 247.5°C. Therefore, if the pressure of the gas increases to 724 torr, the equivalent temperature in degrees Celsius would be approximately 247.5°C.
Learn more about Gay-Lussac's law