Question

One mole of an ideal gas is sealed in a 22.4-l container at a pressure of 1 atm and a temperature of 273 k. the temperature is then increased to 301 k , but the container does not expand. what will the new pressure be?

Answer 1

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


`(P_(1))/(T_(1)) = (P_(2))/(T_(2))`

where P₁ & P₂ are the pressures and T₁ & T₂ are the temperatures of the system.

Using the values provided, we have


`(1)/(P_(2)) = (273)/(301)`

`P_(2) = (301)/(273)`

`P_(2) = 1.10`

Therefore, the new pressure has a value of 1.10 atm.

Answer: 1.10 atm