Final answer:
To determine the final temperature when pressure increases from 1.00 atm to 1.25 atm, we use the direct proportionality of pressure and temperature from the ideal gas law. The initial temperature of 0 degrees Celsius is first converted to Kelvin (273.15 K), and the final temperature is then calculated and converted back to Celsius, resulting in approximately 68.29°C.
Step-by-step explanation:
To find the temperature when the pressure changes from 1.00 atm to 1.25 atm while assuming constant volume and amount of gas, we can use the ideal gas law, which is expressed as PV = nRT. Since we are looking for the final temperature (T2) and we have the initial temperature (T1) at 0 degrees Celsius, which is 273.15 K (Kelvin), we can use the direct proportionality of pressure and temperature given by the equation:
P1/T1 = P2/T2
First, convert the initial temperature to Kelvin:
T1 = 0°C + 273.15 = 273.15 K
Then, plug in the known values to find the final temperature:
T2 = (P2 × T1) / P1
T2 = (1.25 atm × 273.15 K) / 1.00 atm
T2 = 341.44 K
Converting back to Celsius:
T2 = 341.44 K - 273.15
T2 = 68.29°C
Thus, the final temperature when the pressure increases to 1.25 atm is approximately 68.29°C.