An empty aerosol-spray can at room temper mature (20°C) is thrown into an incinerator where the temperature reaches 576°C. If the gas inside the empty container was initially at a pressure of 1 atm, what pressure did it reach inside the incinerator? Assume the gas was at constant volume and the can did not explode. Answer in units of atm.

Question

An empty aerosol-spray can at room temper mature (20°C) is thrown into an incinerator where the temperature reaches 576°C. If the gas inside the empty container was initially at a pressure of 1 atm, what pressure did it reach inside the incinerator? Assume the gas was at constant volume and the can did not explode. Answer in units of atm.

Answer 1

the pressure is proportional to the absolute (Kelvin) temperature

(576 + 273) / (20 + 273) = p / (1 atm)

Answer 2

To solve this question, we can use the Ideal Gas Law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, let's convert the temperatures to Kelvin. Room temperature is 20°C, which is 20 + 273.15 = 293.15 K. The temperature inside the incinerator is 576°C, which is 576 + 273.15 = 849.15 K.

Since the can is empty, there is no gas inside, which means the number of moles (n) is zero.

Now we can rearrange the equation PV = nRT to solve for the pressure (P):

P = nRT / V

As given in the question, the volume (V) remains constant. Therefore, the equation simplifies to:

P = nR(T / V)

Since the number of moles (n) is zero, the pressure (P) inside the incinerator would also be zero.

Therefore, the pressure inside the incinerator would be 0 atm.