F2 (g) <--> 2 F (g)
A 1.00 mol sample of F2 is placed in a 100. L container at 1000K. What is the pressure of the F2 before any decomposes?
To find the pressure of F2 before any decomposition, we need to use the ideal gas law equation:
PV = nRT
where:
P is the pressure in atm,
V is the volume in liters,
n is the number of moles,
R is the ideal gas constant (0.0821 L.atm/mol.K), and
T is the temperature in Kelvin.
In this case, we have a 1.00 mol sample of F2 (n = 1.00 mol) placed in a 100. L container at 1000K. We can substitute these values into the ideal gas law equation:
PV = nRT
P * 100. L = (1.00 mol) * (0.0821 L.atm/mol.K) * 1000K
Simplifying the equation:
P = (1.00 mol) * (0.0821 L.atm/mol.K) * 1000K / 100. L
Calculating the expression:
P = 8.21 atm
Therefore, the pressure of F2 before any decomposition in a 100. L container at 1000K is 8.21 atm.