Question

What is the pressure inside a 750 mL can of deodorant that starts at 15 degrees Celsius and 1.0 atm if the temperature is raised to 95 degrees Celsius?

Answer 1

The final pressure inside the 750 mL can of deodorant, when the temperature is raised to 95 degrees Celsius, is 1.19 atm.

Step-by-step explanation:

To find the final pressure inside the 750 mL can of deodorant after the temperature is raised to 95 degrees Celsius, we can use the ideal gas law formula: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. First, convert the initial temperature and pressure to Kelvin by adding 273.15: T1 = 15 + 273.15 = 288.15 K and P1 = 1.0 atm.

Next, use the combined gas law formula: P1V1/T1 = P2V2/T2, where V2 is the final volume (750 mL) and T2 is the final temperature (95 + 273.15 = 368.15 K). Rearrange the formula to solve for P2: P2 = (P1 * V1 * T2) / (V2 * T1). Plug in the values and calculate the final pressure: P2 = (1.0 atm * 750 mL * 368.15 K) / (750 mL * 288.15 K) = 1.19 atm.

Answer 2

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.