I understand there is a relationship between temperature & pressure. If a rigid open container was placed in a freezer at -15 degrees C. Removed and its airtight cover replaced simultaneously at 1000mb. What would the pressure be within the container if it was kept in a room with an ambilent temperature of 40 degrees C.
Thanks
Mike
If you cover an open cold container after removing it from the freezer, warm air at 313 K and P = 1000 mb will come in contact with the contents, and (after sealing with a lid) chill at constant volume to 258 K.
Since P/T = constant in this case, you end up with a pressure P' that satisfies the equation
P'/258 = Po/313, where Po = 1000 mb
P' = 258/313 * 1000 = 824 mb
Note that I had to use Kelvin temperatures.
Thanks drwls but I cannot read your answer due to adverts on the site covering your typing.
Mike
To find the pressure within the container when kept in a room with an ambient temperature of 40 degrees C, we can use the ideal gas law. The ideal gas law states that the pressure, volume, and temperature of a gas are related by the equation:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
In this case, the container is rigid, which means its volume remains constant. Therefore, we can rewrite the equation as:
P1/T1 = P2/T2
Where P1 is the initial pressure at -15 degrees C, T1 is the initial temperature in Kelvin, P2 is the final pressure at 40 degrees C, and T2 is the final temperature in Kelvin.
First, we need to convert the temperatures from Celsius to Kelvin:
T1 = -15 + 273.15 = 258.15 Kelvin
T2 = 40 + 273.15 = 313.15 Kelvin
Next, we can use the equation to find the final pressure:
P2 = (P1 * T2) / T1
= (1000 * 313.15) / 258.15
By plugging in the values, we get:
P2 = 1210.75 mb
Therefore, the pressure within the container, when kept in a room with an ambient temperature of 40 degrees C, would be approximately 1210.75 millibars.