Suppose a can of aerosol contains a residual amount of gas at pressure of 755mm Hg and a temperature of 25C. What would the presure be if the can were to be heated to 1155c?
Didn't Bob Pursley do this yesterday?
(P1/T1) = (P2/T2)
Remember T must be in kelvin.
To calculate the new pressure of the can after it is heated, we can use the ideal gas law equation, which is:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
In this case, we can assume that the volume and the number of moles of gas inside the can remain constant. So we can rewrite the equation as:
P1/T1 = P2/T2
Where:
P1 = initial pressure
T1 = initial temperature
P2 = final pressure (what we want to find)
T2 = final temperature
Now, let's plug in the given values:
P1 = 755 mm Hg
T1 = 25°C = 25 + 273 = 298 K
T2 = 1155°C = 1155 + 273 = 1428 K
Now, rearrange the equation to solve for P2:
P2 = (P1 * T2) / T1
Substituting the values:
P2 = (755 * 1428) / 298
Now we can calculate:
P2 ≈ 3620 mm Hg
Therefore, if the can were to be heated to 1155°C, the pressure inside the can would be approximately 3620 mm Hg.