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 the F2 gas before any decomposition occurs, you need to use the ideal gas law equation, which is:

PV = nRT

where P is the pressure, V is the volume of the container, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

In this scenario, you are given the volume of the container (100 L), the number of moles of F2 gas (1.00 mol), and the temperature (1000 K). The ideal gas constant, R, is a constant value equal to 0.0821 L·atm/(mol·K).

Now you can plug in the values into the ideal gas law equation and solve for P:

P * 100 L = 1.00 mol * 0.0821 L·atm/(mol·K) * 1000 K

P * 100 L = 82.1 L·atm

Divide both sides of the equation by 100 L to isolate P:

P = 82.1 L·atm / 100 L

P = 0.821 atm

Therefore, the pressure of the F2 gas before any decomposition occurs is 0.821 atm.