When the temperature is -13 degrees Celsius, the air pressure in a tier is 1.5 atm . If the volume does not change, what will the pressure be after the tier has warmed to 13 degrees Celsius?

Answer 1

To find the new pressure, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature in Kelvin

First, we need to convert the temperatures to Kelvin:
-13 degrees Celsius = 260 K
13 degrees Celsius = 286 K

Since the volume does not change, we can set up the equation:

P1/T1 = P2/T2

Plugging in the values we know:
(1.5 atm) / (260 K) = P2 / (286 K)

Now we can solve for P2:
P2 = (1.5 atm) * (286 K) / (260 K)
P2 = 1.65 atm

Therefore, the pressure in the tier will be 1.65 atm after it has warmed to 13 degrees Celsius.