Since the container did not expand despite the change, this means that volume was constant during the process. Gay-Lussac's law states that for ideal gases with constant volume, pressure and temperature are directly proportional.
Mathematically, we have
[tex] \frac{P_{1}}{T_{1}} = \frac{P_{2}}{T_{2}} [/tex]
where P₁ & P₂ are the pressures and T₁ & T₂ are the temperatures of the system.
Using the values provided, we have
[tex] \frac{1}{P_{2}} = \frac{273}{301} [/tex]
[tex] P_{2} = \frac{301}{273} [/tex]
[tex] P_{2} = 1.10 [/tex]
Therefore, the new pressure has a value of 1.10 atm.
Answer: 1.10 atm
