A compartment measures 3.5 meters by 5.5 meters and is 3 meters high. A fire raises the temperature from 68 degrees F to 1500 degrees F. If the starting pressure was 1 atmosphere, what volume is present at the elevated temperature assuming the compartment has openings to reduce pressure?

The volume of the compartment did not change.

If it is the volume of gas you want including that outside, well one would have to assume a temperature for the gas that escaped to outside.

In other words I do not understand the question.

I believe the question has to do with pressure and measurement.

To find the volume present at the elevated temperature, we can use the ideal gas law equation, which states:

PV = nRT

Where:
P is the pressure (in atmospheres)
V is the volume (in liters)
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/mol·K)
T is the temperature (in Kelvin)

Before we proceed with the calculation, we need to convert the given temperatures from Fahrenheit to Kelvin. The relationship between Fahrenheit and Kelvin is given by:

K = (°F - 32) * 5/9 + 273.15

Initial temperature (Ti) in Kelvin:
Ti = (68 - 32) * 5/9 + 273.15

Final temperature (Tf) in Kelvin:
Tf = (1500 - 32) * 5/9 + 273.15

Now, let's calculate the initial and final volumes using the given dimensions of the compartment.

Initial volume (Vi) = length * width * height
Vi = 3.5 meters * 5.5 meters * 3 meters

Final volume (Vf) can be calculated using the initial and final temperatures by rearranging the ideal gas law equation:

Vf = Vi * (Tf / Ti)

Substituting the values into the equation, we can calculate the final volume.