The answer is: the pressure inside a can of deodorant is 1.28 atm.
Gay-Lussac's Law: the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature.
p₁/T₁ = p₂/T₂.
p₁ = 1.0 atm.; initial pressure
T₁ = 15°C = 288.15 K; initial temperature.
T₂ = 95°C = 368.15 K, final temperature
p₂ = ?; final presure.
1.0 atm/288.15 K = p₂/368.15 K.
1.0 atm · 368.15 K = 288.15 K · p₂.
p₂ = 368.15 atm·K ÷ 288.15 K.
p₂ = 1.28 atm.
As the temperature goes up, the pressure also goes up and vice-versa.
