V₁/T₁ = V₂/T₂
Where:
* V₁ is the initial volume
* T₁ is the initial temperature (in Kelvin)
* V₂ is the final volume
* T₂ is the final temperature (in Kelvin)
Explanation:
* As the temperature of an ideal gas increases, the average kinetic energy of the gas molecules increases.
* This increased kinetic energy causes the molecules to move faster and collide with the walls of the container more frequently and with greater force.
* To maintain constant pressure, the volume of the container must increase to accommodate the greater force of the collisions.
Therefore, at constant pressure, if you increase the temperature of 1 mole of an ideal gas, its volume will increase proportionally.
