To solve this problem, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
We can assume that the number of moles of gas (n) and the volume of the container (V) remain constant throughout the process, as it is not mentioned otherwise in the problem.
First, let's convert the initial temperature from degrees Celsius to Kelvin: Initial temperature, T1 = 0°C + 273.15 = 273.15 K
Now we can set up the equation for the initial state: P1 = 2 atm T1 = 273.15 K
Next, let's determine the final temperature (T2) when the pressure inside the container is 2.75 atm.
P2 = 2.75 atm
We need to find T2, so let's rearrange the ideal gas law equation to solve for T: T2 = (P2 * V) / (n * R)
Since n, V, and R are constant, we can simplify the equation to: T2 = (P2 / P1) * T1
Plugging in the values, we get: T2 = (2.75 atm / 2 atm) * 273.15 K T2 ≈ 410.73 K
Therefore, the temperature inside the container will be approximately 410.73 Kelvin (or 137.58°C) when the pressure is 2.75 atm.