A constant pressure tank is filled with air at 16.7 Atm at 24C it warms to 65C, what is the tank pressure
What am I missing here? If it's a constant pressure tank won't the final P be 16.7 atm?
To determine the new tank pressure, we can use the ideal gas law, which states that the pressure (P), volume (V), and temperature (T) of a gas are related as follows: P1 x V1 / T1 = P2 x V2 / T2.
In this case, we are given the initial pressure (P1 = 16.7 atm), the initial temperature (T1 = 24°C + 273.15 = 297.15 K), and the final temperature (T2 = 65°C + 273.15 = 338.15 K).
Since the volume remains constant (constant pressure tank), we can simplify the equation to: P1 / T1 = P2 / T2.
Rearranging the equation to solve for P2, we have: P2 = P1 * T2 / T1.
Substituting the given values into the equation, we get: P2 = 16.7 atm * 338.15 K / 297.15 K.
Calculating this multiplication, we find: P2 ≈ 19.0 atm.
Therefore, the tank pressure when it warms to 65°C is approximately 19.0 atm.