A gas with an initial of 1300 torr at 144 degrees Celsius is cooled to 0 degrees Celsius. Calculate the final pressure, in mmHg.
Is there a chemical formula for calculating final pressure? If so, what is it?
(P1/T1) = (P2/T2)
P in torr is the same as P in mm Hg.
Don't forget to convert T from Celsius to kelvin. K = degrees C + 273.15
To solve this problem, you can use the ideal gas law, which states:
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
T is the temperature in Kelvin
First, you need to convert the temperatures from degrees Celsius to Kelvin. The conversion is given by:
T(K) = T(°C) + 273.15
So, the initial temperature (T1) is 144°C + 273.15 = 417.15 K, and the final temperature (T2) is 0°C + 273.15 = 273.15 K.
Next, you'll need to convert the initial pressure from torr to mmHg. Since 1 torr is equal to 1 mmHg, the initial pressure (P1) remains the same.
Now, you can set up the equation using the initial and final conditions:
P1V1 / T1 = P2V2 / T2
Since the volume (V1) and the number of moles of gas (n) remain constant, they cancel out from the equation.
Substituting the given values:
P1 / T1 = P2 / T2
P2 = (P1 * T2) / T1
Calculating:
P2 = (1300 torr * 273.15 K) / 417.15 K
P2 ≈ 849.93 mmHg
Therefore, the final pressure, in mmHg, is approximately 849.93 mmHg.